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Deck 17: Equilibrium the Extent of Chemical Reactions
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Question
What is the mass-action expression, p, for the following reaction? SbF5(g) + 4Cl2(g) 
SbCl3(g) + 5ClF(g)
A)
B)
C)
D)
E) None of these choices are correct.
SbCl3(g) + 5ClF(g)A)
B)
C)
D)
E) None of these choices are correct.
Question
What is the mass-action expression, 
c, for the following chemical reaction? PbO(s) + CO(g) 
Pb(l) + CO2(g)
A)
B)
C)
D)
E) None of these choices are correct.
c, for the following chemical reaction? PbO(s) + CO(g) Pb(l) + CO2(g)A)
B)
C)
D)
E) None of these choices are correct.
Question
Question
Write the mass-action expression, c, for the following chemical reaction. 3ClO2-(aq) 2ClO3-(aq) + Cl-(aq)
A)
B)
C)
D)
E)
A)
B)
C)
D)
E)
Question
Question
Write the mass-action expression, 
c, for the following chemical reaction. Zn(s) + 2Ag+(aq) 
Zn2+(aq) + 2Ag(s)
A)
B)
C)
D)
E)
c, for the following chemical reaction. Zn(s) + 2Ag+(aq) Zn2+(aq) + 2Ag(s)A)
B)
C)
D)
E)
Question
Question
Write the mass-action expression, 
c, for the following chemical reaction equation.
2C6H6(g) + 15O2(g)
12CO2(g) + 6H2O(g)
A)
B)
C)
D)
E)
c, for the following chemical reaction equation.
2C6H6(g) + 15O2(g)
12CO2(g) + 6H2O(g)A)
B)
C)
D)
E)
Question
The reaction quotient, 
c, for a reaction has a value of 75 while the equilibrium constant, Kc, has a value of 195. Which of the following statements is accurate?
A) The reaction must proceed to the left to establish equilibrium.
B) The reaction must proceed to the right to establish equilibrium.
C) The concentrations of the products will be much smaller than the concentrations of the reactants when the system is at equilibrium.
D) The concentrations of the products will be about the same as the concentrations of the reactants when the system is at equilibrium.
E) None of these choices are correct.
c, for a reaction has a value of 75 while the equilibrium constant, Kc, has a value of 195. Which of the following statements is accurate?A) The reaction must proceed to the left to establish equilibrium.
B) The reaction must proceed to the right to establish equilibrium.
C) The concentrations of the products will be much smaller than the concentrations of the reactants when the system is at equilibrium.
D) The concentrations of the products will be about the same as the concentrations of the reactants when the system is at equilibrium.
E) None of these choices are correct.
Question
Carbon monoxide and chlorine combine in an equilibrium reaction to produce the highly toxic product, phosgene (COCl2) CO(g) + Cl2(g) ![<strong>Carbon monoxide and chlorine combine in an equilibrium reaction to produce the highly toxic product, phosgene (COCl<sub>2</sub>) CO(g) + Cl<sub>2</sub>(g) COCl<sub>2</sub>(g) If the equilibrium constant for this reaction is K<sub>c</sub> = 248, predict, if possible, what will happen when the reactants and product are combined with the concentrations shown. [CO] = [Cl<sub>2</sub>] = 0.010 M; [COCl<sub>2</sub>] = 0.070 M</strong> A) The reaction will proceed to the right. B) The reaction will proceed to the left. C) The reaction is at equilibrium, and no change in concentrations will occur. D) The container volume needs to be specified before a prediction can be made. E) The temperature needs to be specified before a prediction can be made. <div style=padding-top: 35px>](https://d2lvgg3v3hfg70.cloudfront.net/TB7800/11eac68a_1c54_fea7_a448_f7bc933f3b4a_TB7800_11.jpg)
COCl2(g)
If the equilibrium constant for this reaction is Kc = 248, predict, if possible, what will happen when the reactants and product are combined with the concentrations shown.
[CO] = [Cl2] = 0.010 M; [COCl2] = 0.070 M
A) The reaction will proceed to the right.
B) The reaction will proceed to the left.
C) The reaction is at equilibrium, and no change in concentrations will occur.
D) The container volume needs to be specified before a prediction can be made.
E) The temperature needs to be specified before a prediction can be made.
COCl2(g)If the equilibrium constant for this reaction is Kc = 248, predict, if possible, what will happen when the reactants and product are combined with the concentrations shown.
[CO] = [Cl2] = 0.010 M; [COCl2] = 0.070 M
A) The reaction will proceed to the right.
B) The reaction will proceed to the left.
C) The reaction is at equilibrium, and no change in concentrations will occur.
D) The container volume needs to be specified before a prediction can be made.
E) The temperature needs to be specified before a prediction can be made.
Question
Question
Question
Write the mass-action expression, c, for the following chemical reaction. 2Cu2+(aq) + 4I-(aq) 
2CuI(s) + I2(aq)
A)
B)
C)
D)
E)
2CuI(s) + I2(aq)A)
B)
C)
D)
E)
Question
What is the mass-action expression, 
c, for the following chemical reaction? Cu2+(aq) + 4NH3(aq) 
Cu(NH3)42+(aq)
A)
B)
C)
D)
E) None of these choices are correct.
c, for the following chemical reaction? Cu2+(aq) + 4NH3(aq) Cu(NH3)42+(aq)A)
B)
C)
D)
E) None of these choices are correct.
Question
When a chemical system is at equilibrium,
A) the concentrations of the reactants are equal to the concentrations of the products.
B) the concentrations of the reactants and products have reached constant values.
C) the forward and reverse reactions have stopped.
D) the reaction quotient,
, has reached a maximum.
E) the reaction quotient,
, has reached a minimum.
A) the concentrations of the reactants are equal to the concentrations of the products.
B) the concentrations of the reactants and products have reached constant values.
C) the forward and reverse reactions have stopped.
D) the reaction quotient,
, has reached a maximum.E) the reaction quotient,
, has reached a minimum. Question
Question
Carbon monoxide and chlorine combine in an equilibrium reaction to produce the highly toxic product, phosgene (COCl2) CO(g) + Cl2(g) ![<strong>Carbon monoxide and chlorine combine in an equilibrium reaction to produce the highly toxic product, phosgene (COCl<sub>2</sub>) CO(g) + Cl<sub>2</sub>(g) COCl<sub>2</sub>(g) If the equilibrium constant for this reaction is Kc = 248, predict, if possible, what will happen when the reactants and product are combined with the concentrations shown. [CO] = [Cl<sub>2</sub>] = 0.0200 M; [COCl<sub>2</sub>] = 0.0992 M</strong> A) The reaction will proceed to the right. B) The reaction will proceed to the left. C) The reaction is at equilibrium, and no change in concentrations will occur. D) The container volume needs to be specified before a prediction can be made. E) The temperature needs to be specified before a prediction can be made. <div style=padding-top: 35px>](https://d2lvgg3v3hfg70.cloudfront.net/TB7800/11eac68a_1c55_25b8_a448_8fd782737c46_TB7800_11.jpg)
COCl2(g)
If the equilibrium constant for this reaction is Kc = 248, predict, if possible, what will happen when the reactants and product are combined with the concentrations shown.
[CO] = [Cl2] = 0.0200 M; [COCl2] = 0.0992 M
A) The reaction will proceed to the right.
B) The reaction will proceed to the left.
C) The reaction is at equilibrium, and no change in concentrations will occur.
D) The container volume needs to be specified before a prediction can be made.
E) The temperature needs to be specified before a prediction can be made.
COCl2(g)If the equilibrium constant for this reaction is Kc = 248, predict, if possible, what will happen when the reactants and product are combined with the concentrations shown.
[CO] = [Cl2] = 0.0200 M; [COCl2] = 0.0992 M
A) The reaction will proceed to the right.
B) The reaction will proceed to the left.
C) The reaction is at equilibrium, and no change in concentrations will occur.
D) The container volume needs to be specified before a prediction can be made.
E) The temperature needs to be specified before a prediction can be made.
Question
Write the mass-action expression, 
c, for the following chemical reaction. Fe3+(aq) + 3OH-(aq) 
Fe(OH)3(s)
A)
B)
C)
D)
E)
c, for the following chemical reaction. Fe3+(aq) + 3OH-(aq) Fe(OH)3(s)A)
B)
C)
D)
E)
Question
Consider the equilibrium reaction shown below. B2(g) 
2B(g)
If the rate constants are: kfwd = 7.00 × 10-5s-1 and krev = 2.00 × 10-5 L mol-1 s-1, what is the value of Kc under these conditions?
A) 1.75 × 105
B) 3.50
C) 0.286
D) 5.71 × 10-6
E) 1.40 × 10-10
2B(g)If the rate constants are: kfwd = 7.00 × 10-5s-1 and krev = 2.00 × 10-5 L mol-1 s-1, what is the value of Kc under these conditions?
A) 1.75 × 105
B) 3.50
C) 0.286
D) 5.71 × 10-6
E) 1.40 × 10-10
Question
Write the mass-action expression, 
c, for the following chemical reaction. NO(g) + ½Br2(g) 
NOBr(g)
A)
B)
C)
D)
E)
c, for the following chemical reaction. NO(g) + ½Br2(g) NOBr(g)A)
B)
C)
D)
E)
Question
Consider the following two equilibria and their respective equilibrium constants: (1) NO(g) + ½O2(g) 
NO2(g)
(2) 2NO2(g)
2NO(g) + O2(g)
Which one of the following is the correct relationship between the equilibrium constants K1 and K2?
A) K2 = 2/K1
B) K2 = (1/K1)2
C) K2 = -K1/2
D) K2 = 1/(2K1)
E) K2 = 1/(2K1)2
NO2(g)(2) 2NO2(g)
2NO(g) + O2(g)Which one of the following is the correct relationship between the equilibrium constants K1 and K2?
A) K2 = 2/K1
B) K2 = (1/K1)2
C) K2 = -K1/2
D) K2 = 1/(2K1)
E) K2 = 1/(2K1)2
Question
Write the mass-action expression, 
c, for the following chemical reaction. Sn2+(aq) + ½O2(g) + 3H2O(l) 
SnO2(s) + 2H3O+(aq)
A)
B)
C)
D)
E) None of these choices are correct.
c, for the following chemical reaction. Sn2+(aq) + ½O2(g) + 3H2O(l) SnO2(s) + 2H3O+(aq)A)
B)
C)
D)
E) None of these choices are correct.
Question
The equilibrium constant for reaction (1) below is 276. Under the same conditions, what is the equilibrium constant of reaction (2)? (1) ½X2(g) + ½Y2(g) 
XY(g)
(2) 2XY(g)
X2(g) + Y2(g)
A) 6.02 × 10-2
B) 7.25 × 10-3
C) 3.62 × 10-3
D) 1.31 × 10-5
E) None of these choices are correct.
XY(g)(2) 2XY(g)
X2(g) + Y2(g)A) 6.02 × 10-2
B) 7.25 × 10-3
C) 3.62 × 10-3
D) 1.31 × 10-5
E) None of these choices are correct.
Question
The equilibrium constant, Kc, for the decomposition of COBr2 COBr2(g) 
CO(g) + Br2(g)
Is 0.190. What is Kc for the following reaction?
2CO(g) + 2Br2(g)
2COBr2(g)
A) 0.0361
B) 2.63
C) 5.62
D) 10.5
E) 27.7
CO(g) + Br2(g)Is 0.190. What is Kc for the following reaction?
2CO(g) + 2Br2(g)
2COBr2(g)A) 0.0361
B) 2.63
C) 5.62
D) 10.5
E) 27.7
Question
The equilibrium constant, Kp, for the reaction H2(g) + I2(g) 
2HI(g)
Is 55.2 at 425°C. A rigid cylinder at that temperature contains 0.127 atm of hydrogen, 0.134 atm of iodine, and 1.055 atm of hydrogen iodide. Is the system at equilibrium?
A) Yes.
B) No, the forward reaction must proceed to establish equilibrium.
C) No, the reverse reaction must proceed to establish equilibrium.
D) Need to know the volume of the container before deciding.
E) Need to know the starting concentrations of all substances before deciding.
2HI(g)Is 55.2 at 425°C. A rigid cylinder at that temperature contains 0.127 atm of hydrogen, 0.134 atm of iodine, and 1.055 atm of hydrogen iodide. Is the system at equilibrium?
A) Yes.
B) No, the forward reaction must proceed to establish equilibrium.
C) No, the reverse reaction must proceed to establish equilibrium.
D) Need to know the volume of the container before deciding.
E) Need to know the starting concentrations of all substances before deciding.
Question
What is the mass-action expression, 
c, for the following chemical reaction? 4H3O+(aq) + 2Cl-(aq) + MnO2(s) 
Mn2+(aq) + 6H2O(l) + Cl2(g)
A)
B)
C)
D)
E) None of these choices are correct.
c, for the following chemical reaction? 4H3O+(aq) + 2Cl-(aq) + MnO2(s) Mn2+(aq) + 6H2O(l) + Cl2(g)A)
B)
C)
D)
E) None of these choices are correct.
Question
The reaction of nitrogen with oxygen to form nitrogen monoxide can be represented by the following equation. N2(g) + O2(g) 
2NO(g)
At 2000°C, the equilibrium constant, Kc, has a value of 4.10 × 10-4. What is the value of Kp?
A) 2.17 × 10-8
B) 4.10 × 10-4
C) 7.65 × 10-2
D) 7.75
E) None of these choices are correct.
2NO(g)At 2000°C, the equilibrium constant, Kc, has a value of 4.10 × 10-4. What is the value of Kp?
A) 2.17 × 10-8
B) 4.10 × 10-4
C) 7.65 × 10-2
D) 7.75
E) None of these choices are correct.
Question
Write the mass-action expression, 
c, for the following chemical reaction. MgO(s) + SO2(g) + ½O2(g) 
MgSO4(s)
A)
B)
C)
D)
E) None of these choices are correct.
c, for the following chemical reaction. MgO(s) + SO2(g) + ½O2(g) MgSO4(s)A)
B)
C)
D)
E) None of these choices are correct.
Question
Nitrogen dioxide decomposes according to the reaction 2NO2(g) 
2NO(g) + O2(g)
Where Kp = 4.48 × 10-13 at 25°C. What is the value for Kc?
A) 1.81 × 10-16
B) 1.83 × 10-14
C) 4.48 × 10-13
D) 1.10 × 10-11
E) 1.11 × 10-9
2NO(g) + O2(g)Where Kp = 4.48 × 10-13 at 25°C. What is the value for Kc?
A) 1.81 × 10-16
B) 1.83 × 10-14
C) 4.48 × 10-13
D) 1.10 × 10-11
E) 1.11 × 10-9
Question
Consider the equilibrium reaction: H2(g) + Br2(g) 
2HBr(g) Which of the following correctly describes the relationship between Kc and Kp for the reaction?
A) Kp = Kc
B) Kp = (RT)Kc
C) Kp = (RT)2Kc
D) Kp = Kc / RT
E) Kp = Kc / (RT)2
2HBr(g) Which of the following correctly describes the relationship between Kc and Kp for the reaction?A) Kp = Kc
B) Kp = (RT)Kc
C) Kp = (RT)2Kc
D) Kp = Kc / RT
E) Kp = Kc / (RT)2
Question
About half of the sodium carbonate produced is used in making glass products because it lowers the melting point of sand, the major component of glass. When sodium carbonate is added to water it hydrolyses according to the following reactions. CO32-(aq) + H2O(l) 
HCO3-(aq) + OH-(aq) K1
HCO3(aq) + H2O(l)
H2CO3(aq) + OH-(aq) K2
These can be combined to yield
CO32-(aq) + 2H2O(l)
H2CO3(aq) + 2OH-(aq) K3
What is the value of K3?
A) K1 × K2
B) K1 ÷ K2
C) K1 + K2
D) K1 - K2
E) (K1K2)2
HCO3-(aq) + OH-(aq) K1HCO3(aq) + H2O(l)
H2CO3(aq) + OH-(aq) K2These can be combined to yield
CO32-(aq) + 2H2O(l)
H2CO3(aq) + 2OH-(aq) K3What is the value of K3?
A) K1 × K2
B) K1 ÷ K2
C) K1 + K2
D) K1 - K2
E) (K1K2)2
Question
N2(g) + O2(g) 
2NO(g) Kc = 4.8 × 10-31 2NOBr(g) 
2NO(g) + Br2(g) Kc = 0.50
Given the above equilibrium constant data at 25°C, what is the value of Kc at this temperature for the reaction
2NOBr(g)
N2(g) + O2(g) + Br2(g)?
A) 2.4 × 10-31
B) 9.6 × 10-31
C) 1.0 × 1030
D) 4.2 × 1030
E) None of these choices are correct.
2NO(g) Kc = 4.8 × 10-31 2NOBr(g) 2NO(g) + Br2(g) Kc = 0.50Given the above equilibrium constant data at 25°C, what is the value of Kc at this temperature for the reaction
2NOBr(g)
N2(g) + O2(g) + Br2(g)?A) 2.4 × 10-31
B) 9.6 × 10-31
C) 1.0 × 1030
D) 4.2 × 1030
E) None of these choices are correct.
Question
The equilibrium constant for the reaction of bromine with chlorine to form bromine monochloride is 58.0 at a certain temperature. Br2(g) + Cl2(g) 
2BrCl(g)
What is the equilibrium constant for the following reaction?
BrCl(g)
½Br2(g) + ½Cl2(g)
A) 2.97 × 10-4
B) 1.72 × 10-2
C) 3.45 × 10-2
D) 1.31 × 10-1
E) > 1.00
2BrCl(g)What is the equilibrium constant for the following reaction?
BrCl(g)
½Br2(g) + ½Cl2(g)A) 2.97 × 10-4
B) 1.72 × 10-2
C) 3.45 × 10-2
D) 1.31 × 10-1
E) > 1.00
Question
The equilibrium constant, Kp, has a value of 6.5 × 10-4 at 308 K for the reaction of nitrogen monoxide with chlorine. 2NO(g) + Cl2(g) 
2NOCl(g)
What is the value of Kc?
A) 2.5 × 10-7
B) 6.5 × 10-4
C) 1.6 × 10-2
D) 1.7
E) None of these choices are correct.
2NOCl(g)What is the value of Kc?
A) 2.5 × 10-7
B) 6.5 × 10-4
C) 1.6 × 10-2
D) 1.7
E) None of these choices are correct.
Question
H2SO3(aq) 
HSO3(aq) + H+(aq) Kc = 1.4 × 10-2 H2SO3(aq) 
SO32-(aq) + 2H+(aq) Kc = 9.1 × 10-10
Given the above equilibrium constant data at 25°C, what is the value of Kc at this temperature for the reaction
HSO3-(aq)
SO32-(aq) + H+(aq)?
A) 6.5 ×10-8
B) 1.3 × 10-11
C) 7.8 × 1010
D) 1.5 × 107
E) None of these choices are correct.
HSO3(aq) + H+(aq) Kc = 1.4 × 10-2 H2SO3(aq) SO32-(aq) + 2H+(aq) Kc = 9.1 × 10-10Given the above equilibrium constant data at 25°C, what is the value of Kc at this temperature for the reaction
HSO3-(aq)
SO32-(aq) + H+(aq)?A) 6.5 ×10-8
B) 1.3 × 10-11
C) 7.8 × 1010
D) 1.5 × 107
E) None of these choices are correct.
Question
In water, the following equilibrium exists: H+(aq) + OH-(aq) 
H2O(l)
In pure water at 25°C, the concentration of H+ ions is 1.00 × 10-7 mol/L. Calculate the value of the equilibrium constant for the reaction as written above.
A) 1.00 × 1014
B) 1.00 × 1012
C) 1.00 × 10-14
D) 1.00 × 10-12
E) 5.55 × 1015
H2O(l)In pure water at 25°C, the concentration of H+ ions is 1.00 × 10-7 mol/L. Calculate the value of the equilibrium constant for the reaction as written above.
A) 1.00 × 1014
B) 1.00 × 1012
C) 1.00 × 10-14
D) 1.00 × 10-12
E) 5.55 × 1015
Question
Hydrogen sulfide will react with water as shown in the following reactions. H2S(g) + H2O(l) 
H3O+(aq) + HS-(aq) K1 = 1.0 × 10-7
HS-(aq) + H2O(l)
H3O+(aq) + S2-(aq) K2 = ?
H2S(g) + 2H2O(l)
2H3O+(aq) + S2-(aq) K3 = 1.3 × 10-20
What is the value of K2?
A) 1.3 × 10-27
B) 2.3 × 10-7
C) 1.3 × 10-13
D) 7.7 × 1012
E) 7.7 × 1026
H3O+(aq) + HS-(aq) K1 = 1.0 × 10-7HS-(aq) + H2O(l)
H3O+(aq) + S2-(aq) K2 = ?H2S(g) + 2H2O(l)
2H3O+(aq) + S2-(aq) K3 = 1.3 × 10-20What is the value of K2?
A) 1.3 × 10-27
B) 2.3 × 10-7
C) 1.3 × 10-13
D) 7.7 × 1012
E) 7.7 × 1026
Question
Consider the equilibrium reaction: N2O4(g) 
2NO2(g) Which of the following correctly describes the relationship between Kc and Kp for the reaction?
A) Kp = Kc
B) Kp = RT × Kc
C) Kp = (RT × Kc)-1
D) Kp = Kc / RT
E) Kp = RT / Kc
2NO2(g) Which of the following correctly describes the relationship between Kc and Kp for the reaction?A) Kp = Kc
B) Kp = RT × Kc
C) Kp = (RT × Kc)-1
D) Kp = Kc / RT
E) Kp = RT / Kc
Question
Consider the reactions of cadmium with the thiosulfate anion. Cd2+(aq) + S2O32-(aq) 
Cd(S2O3)(aq) K1 = 8.3 × 103
Cd(S2O3)(aq) + S2O32-(aq)
Cd(S2O3)22-(aq) K2 = 2.5 × 102
What is the value for the equilibrium constant for the following reaction?
Cd2+(aq) + 2S2O32-(aq)
Cd(S2O3)22-(aq)
A) 0.030
B) 33
C) 8.1 × 103
D) 8.6 × 103
E) 2.1 × 106
Cd(S2O3)(aq) K1 = 8.3 × 103Cd(S2O3)(aq) + S2O32-(aq)
Cd(S2O3)22-(aq) K2 = 2.5 × 102What is the value for the equilibrium constant for the following reaction?
Cd2+(aq) + 2S2O32-(aq)
Cd(S2O3)22-(aq)A) 0.030
B) 33
C) 8.1 × 103
D) 8.6 × 103
E) 2.1 × 106
Question
At 500°C the equilibrium constant, Kp, is 4.00 × 10-4 for the equilibrium: 2HCN(g) 
H2(g) + C2N2(g)
What is Kp for the following reaction?
H2(g) + C2N2(g)
2HCN(g)
A) 2.00 × 10-4
B) -4.00 × 10-4
C) 1.25 × 103
D) 2.50 × 103
E) 4.00 × 104
H2(g) + C2N2(g)What is Kp for the following reaction?
H2(g) + C2N2(g)
2HCN(g)A) 2.00 × 10-4
B) -4.00 × 10-4
C) 1.25 × 103
D) 2.50 × 103
E) 4.00 × 104
Question
10.0 mL of a 0.100 mol L-1 solution of a metal ion M2+ is mixed with 10.0 mL of a 0.100 mol L-1 solution of a substance L. The following equilibrium is established: M2+(aq) + 2L(aq) 
ML22+(aq)
At equilibrium the concentration of L is found to be 0.0100 mol L-1. What is the equilibrium concentration of ML22+, in mol L-1?
A) 0.100 mol L-1
B) 0.050 mol L-1
C) 0.025 mol L-1
D) 0.0200 mol L-1
E) 0.0100 mol L-1
ML22+(aq)At equilibrium the concentration of L is found to be 0.0100 mol L-1. What is the equilibrium concentration of ML22+, in mol L-1?
A) 0.100 mol L-1
B) 0.050 mol L-1
C) 0.025 mol L-1
D) 0.0200 mol L-1
E) 0.0100 mol L-1
Question
Nitric oxide and bromine were allowed to react in a sealed container. When equilibrium was reached PNO = 0.526 atm, 
= 1.59 atm, and PNOBr = 7.68 atm. Calculate Kp for the reaction.
2NO(g) + Br2(g)
2NOBr(g)
A) 7.45 × 10-3
B) 0.109
C) 9.18
D) 91.8
E) 134
= 1.59 atm, and PNOBr = 7.68 atm. Calculate Kp for the reaction.2NO(g) + Br2(g)
2NOBr(g)A) 7.45 × 10-3
B) 0.109
C) 9.18
D) 91.8
E) 134
Question
Question
At 850°C, the equilibrium constant Kp for the reaction C(s) + CO2(g) 
2CO(g)
Has a value of 10.7. If the total pressure in the system at equilibrium is 1.000 atm, what is the partial pressure of carbon monoxide?
A) 0.362 atm
B) 0.489 atm
C) 0.667 atm
D) 0.915 atm
E) 0.921 atm
2CO(g)Has a value of 10.7. If the total pressure in the system at equilibrium is 1.000 atm, what is the partial pressure of carbon monoxide?
A) 0.362 atm
B) 0.489 atm
C) 0.667 atm
D) 0.915 atm
E) 0.921 atm
Question
At 25°C, the equilibrium constant Kc for the reaction 2A(aq) 
B(aq) + C(aq)
Is 65. If 2.50 mol of A is added to enough water to prepare 1.00 L of solution, what will the equilibrium concentration of A be?
A) 0.038 M
B) 0.14 M
C) 0.28 M
D) 1.18 M
E) 2.4 M
B(aq) + C(aq)Is 65. If 2.50 mol of A is added to enough water to prepare 1.00 L of solution, what will the equilibrium concentration of A be?
A) 0.038 M
B) 0.14 M
C) 0.28 M
D) 1.18 M
E) 2.4 M
Question
Question
Ammonium iodide dissociates reversibly to ammonia and hydrogen iodide. NH4I(s) 
NH3(g) + HI(g)
At 400°C, Kp = 0.215. Calculate the partial pressure of ammonia at equilibrium when a sufficient quantity of ammonium iodide is heated to 400°C.
A) 0.103 atm
B) 0.215 atm
C) 0.232 atm
D) 0.464 atm
E) 2.00 atm
NH3(g) + HI(g)At 400°C, Kp = 0.215. Calculate the partial pressure of ammonia at equilibrium when a sufficient quantity of ammonium iodide is heated to 400°C.
A) 0.103 atm
B) 0.215 atm
C) 0.232 atm
D) 0.464 atm
E) 2.00 atm
Question
At a certain temperature the reaction CO2(g) + H2(g) 
CO(g) + H2O(g)2
Has Kc = 2.50. If 2.00 mol of carbon dioxide and 1.5 mol of hydrogen are placed in a 5.00 L vessel and equilibrium is established, what will be the concentration of carbon monoxide?
A) 0.091 M
B) 0.191 M
C) 0.209 M
D) 0.913 M
E) 1.05 M
CO(g) + H2O(g)2Has Kc = 2.50. If 2.00 mol of carbon dioxide and 1.5 mol of hydrogen are placed in a 5.00 L vessel and equilibrium is established, what will be the concentration of carbon monoxide?
A) 0.091 M
B) 0.191 M
C) 0.209 M
D) 0.913 M
E) 1.05 M
Question
A mixture of 0.500 mole of carbon monoxide and 0.400 mole of bromine was placed into a rigid 1.00-L container and the system was allowed to come to equilibrium. The equilibrium
Concentration of COBr2 was 0.233 M. What is the value of Kc for this reaction?
CO(g) + Br2(g)
COBr2(g)
A) 5.23
B) 1.22
C) 1.165
D) 0.858
E) 0.191
Concentration of COBr2 was 0.233 M. What is the value of Kc for this reaction?
CO(g) + Br2(g)
COBr2(g)A) 5.23
B) 1.22
C) 1.165
D) 0.858
E) 0.191
Question
The equilibrium constant, Kp, for the reaction CO(g) + H2O(g) 
CO2(g) + H2(g)
At 986°C is 0.63. A rigid cylinder at that temperature contains 1.2 atm of carbon monoxide, 0.20 atm of water vapor, 0.30 atm of carbon dioxide, and 0.27 atm of hydrogen. Is the system at equilibrium?
A) Yes.
B) No, the forward reaction must proceed to establish equilibrium.
C) No, the reverse reaction must proceed to establish equilibrium.
D) Need to know the volume of the container before deciding.
E) Need to know the starting concentrations of all substances before deciding.
CO2(g) + H2(g)At 986°C is 0.63. A rigid cylinder at that temperature contains 1.2 atm of carbon monoxide, 0.20 atm of water vapor, 0.30 atm of carbon dioxide, and 0.27 atm of hydrogen. Is the system at equilibrium?
A) Yes.
B) No, the forward reaction must proceed to establish equilibrium.
C) No, the reverse reaction must proceed to establish equilibrium.
D) Need to know the volume of the container before deciding.
E) Need to know the starting concentrations of all substances before deciding.
Question
The equilibrium constant Kc for the reaction PCl3(g) + Cl2(g) 
PCl5(g)
Is 49 at 230°C. If 0.70 mol of PCl3 is added to 0.70 mol of Cl2 in a 1.00-L reaction vessel at 230°C, what is the concentration of PCl3 when equilibrium has been established?
A) 0.049 M
B) 0.11 M
C) 0.30 M
D) 0.59 M
E) 0.83 M
PCl5(g)Is 49 at 230°C. If 0.70 mol of PCl3 is added to 0.70 mol of Cl2 in a 1.00-L reaction vessel at 230°C, what is the concentration of PCl3 when equilibrium has been established?
A) 0.049 M
B) 0.11 M
C) 0.30 M
D) 0.59 M
E) 0.83 M
Question
At high temperatures, carbon reacts with O2 to produce CO as follows: C(s) + O2(g) 
2CO(g).
When 0.350 mol of O2 and excess carbon were placed in a 5.00-L container and heated, the equilibrium concentration of CO was found to be 0.060 M. What is the equilibrium constant, Kc, for this reaction?
A) 0.010
B) 0.072
C) 0.090
D) 0.17
E) 1.2
2CO(g).When 0.350 mol of O2 and excess carbon were placed in a 5.00-L container and heated, the equilibrium concentration of CO was found to be 0.060 M. What is the equilibrium constant, Kc, for this reaction?
A) 0.010
B) 0.072
C) 0.090
D) 0.17
E) 1.2
Question
The equilibrium constant Kc for the reaction A(g) + B(g) 
C(g)
Is 0.76 at 150°C. If 0.800 mol of A is added to 0.600 mol of B in a 1.00-L container at 150°C, what will be the equilibrium concentration of C?
A) 0.19 M
B) 0.29 M
C) 0.36 M
D) 0.41 M
E) 0.51 M
C(g)Is 0.76 at 150°C. If 0.800 mol of A is added to 0.600 mol of B in a 1.00-L container at 150°C, what will be the equilibrium concentration of C?
A) 0.19 M
B) 0.29 M
C) 0.36 M
D) 0.41 M
E) 0.51 M
Question
Compounds A, B, and C react according to the following equation. 3A(g) + 2B(g) ![<strong>Compounds A, B, and C react according to the following equation. 3A(g) + 2B(g) 2C(g) At 100°C a mixture of these gases at equilibrium showed that [A] = 0.855 M, [B] = 1.23 M, and [C] = 1.75 M. What is the value of K<sub>c</sub> for this reaction?</strong> A) 0.309 B) 0.601 C) 1.66 D) 3.24 E) > 10 <div style=padding-top: 35px>](https://d2lvgg3v3hfg70.cloudfront.net/TB7800/11eac68a_1c5f_fa96_a448_153f2af0638d_TB7800_11.jpg)
2C(g)
At 100°C a mixture of these gases at equilibrium showed that [A] = 0.855 M, [B] = 1.23 M, and [C] = 1.75 M. What is the value of Kc for this reaction?
A) 0.309
B) 0.601
C) 1.66
D) 3.24
E) > 10
2C(g)At 100°C a mixture of these gases at equilibrium showed that [A] = 0.855 M, [B] = 1.23 M, and [C] = 1.75 M. What is the value of Kc for this reaction?
A) 0.309
B) 0.601
C) 1.66
D) 3.24
E) > 10
Question
The reaction system POCl3(g) 
POCl(g) + Cl2(g)
Is at equilibrium. Which of the following statements describes the behavior of the system if POCl is added to the container?
A) The forward reaction will proceed to establish equilibrium.
B) The reverse reaction will proceed to establish equilibrium.
C) The partial pressures of POCl3 and POCl will remain steady while the partial pressure of chlorine increases.
D) The partial pressure of chlorine remains steady while the partial pressures of POCl3 and POCl increase.
E) The partial pressure of chlorine will increase while the partial pressure of POCl decreases.
POCl(g) + Cl2(g)Is at equilibrium. Which of the following statements describes the behavior of the system if POCl is added to the container?
A) The forward reaction will proceed to establish equilibrium.
B) The reverse reaction will proceed to establish equilibrium.
C) The partial pressures of POCl3 and POCl will remain steady while the partial pressure of chlorine increases.
D) The partial pressure of chlorine remains steady while the partial pressures of POCl3 and POCl increase.
E) The partial pressure of chlorine will increase while the partial pressure of POCl decreases.
Question
The following reaction, in CCl4 solvent, has been studied at 25°C. 2BrCl 
Br2 + Cl2
The equilibrium constant Kc is known to be 0.141. If the initial concentration of chlorine is 0.0300 M and of bromine monochloride is 0.0200 M, what is the equilibrium concentration of bromine?
A) 1.35 × 10-3 M
B) 2.70 × 10-3 M
C) 8.82 × 10-3 M
D) 9.70 × 10-2 M
E) None of these choices are correct.
Br2 + Cl2The equilibrium constant Kc is known to be 0.141. If the initial concentration of chlorine is 0.0300 M and of bromine monochloride is 0.0200 M, what is the equilibrium concentration of bromine?
A) 1.35 × 10-3 M
B) 2.70 × 10-3 M
C) 8.82 × 10-3 M
D) 9.70 × 10-2 M
E) None of these choices are correct.
Question
At 25°C, the equilibrium constant Kc for the reaction 2A(g) 
B(g) + C(g)
Is 0.035. A mixture of 8.00 moles of B and 12.00 moles of C in a 20.0 L container is allowed to come to equilibrium. What is the equilibrium concentration of A?
A) < 0.100 M
B) 0.339 M
C) 0.678 M
D) 6.78 M
E) 13.56 M
B(g) + C(g)Is 0.035. A mixture of 8.00 moles of B and 12.00 moles of C in a 20.0 L container is allowed to come to equilibrium. What is the equilibrium concentration of A?
A) < 0.100 M
B) 0.339 M
C) 0.678 M
D) 6.78 M
E) 13.56 M
Question
Consider the reversible reaction: 2NO2(g) 
N2O4(g) If the concentrations of both NO2 and N2O4 are 0.016 mol L-1, what is the value of 
c?
A) 0.016
B) 0.50
C) 1.0
D) 2.0
E) 63
N2O4(g) If the concentrations of both NO2 and N2O4 are 0.016 mol L-1, what is the value of c?
A) 0.016
B) 0.50
C) 1.0
D) 2.0
E) 63
Question
A mixture of 0.600 mol of bromine and 1.600 mol of iodine is placed into a rigid 1.000-L container at 350°C. Br2(g) + I2(g) 
2IBr(g)
When the mixture has come to equilibrium, the concentration of iodine monobromide is 1.190 M. What is the equilibrium constant for this reaction at 350°C?
A) 3.55 × 10-3
B) 1.24
C) 1.47
D) 282
E) 325
2IBr(g)When the mixture has come to equilibrium, the concentration of iodine monobromide is 1.190 M. What is the equilibrium constant for this reaction at 350°C?
A) 3.55 × 10-3
B) 1.24
C) 1.47
D) 282
E) 325
Question
Nitric oxide is formed in automobile exhaust when nitrogen and oxygen in air react at high temperatures. N2(g) + O2(g) 
2NO(g)
The equilibrium constant Kp for the reaction is 0.0025 at 2127°C. If a container is charged with 8.00 atm of nitrogen and 5.00 atm of oxygen and the mixture is allowed to reach equilibrium, what will be the equilibrium partial pressure of nitrogen?
A) 0.16 atm
B) 0.31 atm
C) 3.1 atm
D) 7.7 atm
E) 7.8 atm
2NO(g)The equilibrium constant Kp for the reaction is 0.0025 at 2127°C. If a container is charged with 8.00 atm of nitrogen and 5.00 atm of oxygen and the mixture is allowed to reach equilibrium, what will be the equilibrium partial pressure of nitrogen?
A) 0.16 atm
B) 0.31 atm
C) 3.1 atm
D) 7.7 atm
E) 7.8 atm
Question
The reaction system CS2(g) + 4H2(g) 
CH4(g) + 2H2S(g)
Is at equilibrium. Which of the following statements describes the behavior of the system if the partial pressure of hydrogen is doubled?
A) As equilibrium is reestablished, the partial pressure of carbon disulfide increases.
B) As equilibrium is reestablished, the partial pressure of methane, CH4, decreases.
C) As equilibrium is reestablished, the partial pressure of hydrogen decreases.
D) As equilibrium is reestablished, the partial pressure of hydrogen sulfide decreases.
E) As equilibrium is reestablished, all the partial pressures will decrease.
CH4(g) + 2H2S(g)Is at equilibrium. Which of the following statements describes the behavior of the system if the partial pressure of hydrogen is doubled?
A) As equilibrium is reestablished, the partial pressure of carbon disulfide increases.
B) As equilibrium is reestablished, the partial pressure of methane, CH4, decreases.
C) As equilibrium is reestablished, the partial pressure of hydrogen decreases.
D) As equilibrium is reestablished, the partial pressure of hydrogen sulfide decreases.
E) As equilibrium is reestablished, all the partial pressures will decrease.
Question
The following reaction is at equilibrium at one atmosphere, in a closed container. NaOH(s) + CO2(g) 
NaHCO3(s)
Which, if any, of the following actions will decrease the total amount of CO2 gas present at equilibrium?
A) adding N2 gas to double the pressure
B) adding more solid NaOH
C) decreasing the volume of the container
D) removing half of the solid NaHCO3
E) None of these choices are correct.
NaHCO3(s)Which, if any, of the following actions will decrease the total amount of CO2 gas present at equilibrium?
A) adding N2 gas to double the pressure
B) adding more solid NaOH
C) decreasing the volume of the container
D) removing half of the solid NaHCO3
E) None of these choices are correct.
Question
Nitrogen dioxide can dissociate to nitric oxide and oxygen. 2NO2(g) 
2NO(g) + O2(g) ΔH°rxn = +114 kJ
Under which reaction conditions would you expect to produce the largest amount of oxygen?
A) high temperature, high pressure
B) low temperature, high pressure
C) high temperature, low pressure
D) low temperature, low pressure
E) None of these choices are correct.
2NO(g) + O2(g) ΔH°rxn = +114 kJUnder which reaction conditions would you expect to produce the largest amount of oxygen?
A) high temperature, high pressure
B) low temperature, high pressure
C) high temperature, low pressure
D) low temperature, low pressure
E) None of these choices are correct.
Question
Methanol can be synthesized by combining carbon monoxide and hydrogen. CO(g) + 2H2(g) 
CH3OH(g) ΔH°rxn = -90.7 kJ
A reaction vessel contains these compounds at equilibrium. What effect will be seen when equilibrium is re-established after decreasing the temperature by 45°C?
A) All the partial pressures will decrease.
B) The partial pressure of methanol will decrease.
C) The partial pressures of hydrogen and methanol will decrease.
D) The partial pressure of hydrogen will increase.
E) The partial pressure of carbon monoxide will decrease.
CH3OH(g) ΔH°rxn = -90.7 kJA reaction vessel contains these compounds at equilibrium. What effect will be seen when equilibrium is re-established after decreasing the temperature by 45°C?
A) All the partial pressures will decrease.
B) The partial pressure of methanol will decrease.
C) The partial pressures of hydrogen and methanol will decrease.
D) The partial pressure of hydrogen will increase.
E) The partial pressure of carbon monoxide will decrease.
Question
Sodium hydrogen carbonate decomposes above 110°C to form sodium carbonate, water, and carbon dioxide. 2NaHCO3(s) 
Na2CO3(s) + H2O(g) + CO2(g)
One thousand grams of sodium hydrogen carbonate are added to a reaction vessel, the temperature is increased to 200°C, and the system comes to equilibrium. What happens in this system if another 50 g of sodium carbonate are now added?
A) The partial pressure of carbon dioxide will increase.
B) The partial pressure of carbon dioxide will decrease.
C) The partial pressure of carbon dioxide will be unchanged.
D) The amounts of all products will be greater when equilibrium is reestablished.
E) None of these choices are correct.
Na2CO3(s) + H2O(g) + CO2(g)One thousand grams of sodium hydrogen carbonate are added to a reaction vessel, the temperature is increased to 200°C, and the system comes to equilibrium. What happens in this system if another 50 g of sodium carbonate are now added?
A) The partial pressure of carbon dioxide will increase.
B) The partial pressure of carbon dioxide will decrease.
C) The partial pressure of carbon dioxide will be unchanged.
D) The amounts of all products will be greater when equilibrium is reestablished.
E) None of these choices are correct.
Question
Hydrogen sulfide can be formed in the following reaction: H2(g) + ½S2(g) 
H2S(g) ΔH°rxn = -92 kJ
The equilibrium constant Kp = 106 at 1023 K. Estimate the value of Kp at 1218 K.
A) 5.05
B) 18.8
C) 34.7
D) 88.9
E) 598
H2S(g) ΔH°rxn = -92 kJThe equilibrium constant Kp = 106 at 1023 K. Estimate the value of Kp at 1218 K.
A) 5.05
B) 18.8
C) 34.7
D) 88.9
E) 598
Question
The reaction system POCl3(g) 
POCl(g) + Cl2(g)
Is at equilibrium. Which of the following statements describes the behavior of the system if the partial pressure of chlorine is reduced by 50%?
A) POCl3 will be consumed as equilibrium is established.
B) POCl will be consumed as equilibrium is established.
C) Chlorine will be consumed as equilibrium is established.
D) The partial pressure of POCl will decrease while the partial pressure of Cl2 increases as equilibrium is established.
E) The volume will have to decrease before equilibrium can be reestablished.
POCl(g) + Cl2(g)Is at equilibrium. Which of the following statements describes the behavior of the system if the partial pressure of chlorine is reduced by 50%?
A) POCl3 will be consumed as equilibrium is established.
B) POCl will be consumed as equilibrium is established.
C) Chlorine will be consumed as equilibrium is established.
D) The partial pressure of POCl will decrease while the partial pressure of Cl2 increases as equilibrium is established.
E) The volume will have to decrease before equilibrium can be reestablished.
Question
The following reaction is at equilibrium in a closed container. CuSO4.5H2O(s) 
CuSO4(s) + 5H2O(g)
Which, if any, of the following actions will lead to an increase in the pressure of H2O present at equilibrium?
A) increasing the volume of the container
B) decreasing the volume of the container
C) adding a catalyst
D) removing some solid CuSO4
E) None of these choices are correct.
CuSO4(s) + 5H2O(g)Which, if any, of the following actions will lead to an increase in the pressure of H2O present at equilibrium?
A) increasing the volume of the container
B) decreasing the volume of the container
C) adding a catalyst
D) removing some solid CuSO4
E) None of these choices are correct.
Question
Methanol can be synthesized by combining carbon monoxide and hydrogen. CO(g) + 2H2(g) 
CH3OH(g)
A reaction vessel contains the three gases at equilibrium with a total pressure of 1.00 atm. What will happen to the partial pressure of hydrogen if enough argon is added to raise the total pressure to 1.4 atm?
A) The partial pressure of hydrogen will decrease.
B) The partial pressure of hydrogen will increase.
C) The partial pressure of hydrogen will be unchanged.
D) Kp needs to be known before a prediction can be made.
E) Both Kp and the temperature need to be known before a prediction can be made.
CH3OH(g)A reaction vessel contains the three gases at equilibrium with a total pressure of 1.00 atm. What will happen to the partial pressure of hydrogen if enough argon is added to raise the total pressure to 1.4 atm?
A) The partial pressure of hydrogen will decrease.
B) The partial pressure of hydrogen will increase.
C) The partial pressure of hydrogen will be unchanged.
D) Kp needs to be known before a prediction can be made.
E) Both Kp and the temperature need to be known before a prediction can be made.
Question
Magnesium hydroxide is used in several antacid formulations. When it is added to water it dissociates into magnesium and hydroxide ions. Mg(OH)2(s) 
Mg2+(aq) + 2OH-(aq)
The equilibrium constant at 25°C is 8.9 × 10-12. One hundred grams of magnesium hydroxide is added to 1.00 L of water and equilibrium is established. What happens to the solution if another 10 grams of Mg(OH)2 are now added to the mixture?
A) The hydroxide ion concentration will decrease.
B) The hydroxide ion concentration will increase.
C) The hydroxide ion concentration will be unchanged.
D) The solution will become supersaturated.
E) None of these choices are correct.
Mg2+(aq) + 2OH-(aq)The equilibrium constant at 25°C is 8.9 × 10-12. One hundred grams of magnesium hydroxide is added to 1.00 L of water and equilibrium is established. What happens to the solution if another 10 grams of Mg(OH)2 are now added to the mixture?
A) The hydroxide ion concentration will decrease.
B) The hydroxide ion concentration will increase.
C) The hydroxide ion concentration will be unchanged.
D) The solution will become supersaturated.
E) None of these choices are correct.
Question
Hydrogen bromide will dissociate into hydrogen and bromine gases. 2HBr(g) 
H2(g) + Br2(g) ΔH°rxn = 68 kJ
What effect will a temperature increase of 50°C have on this system at equilibrium?
A) The partial pressure of hydrogen bromide will increase.
B) The partial pressure of hydrogen will increase.
C) The partial pressure of hydrogen bromide and bromine will increase.
D) There will be no effect on the partial pressure of any of the gases.
E) Need to know the initial pressure, volume, and temperature before any of the above predictions can be made.
H2(g) + Br2(g) ΔH°rxn = 68 kJWhat effect will a temperature increase of 50°C have on this system at equilibrium?
A) The partial pressure of hydrogen bromide will increase.
B) The partial pressure of hydrogen will increase.
C) The partial pressure of hydrogen bromide and bromine will increase.
D) There will be no effect on the partial pressure of any of the gases.
E) Need to know the initial pressure, volume, and temperature before any of the above predictions can be made.
Question
At 450°C, tert-butyl alcohol decomposes into water and isobutene. (CH3)3COH(g) 
(CH3)2CCH2(g) + H2O(g)
A reaction vessel contains these compounds at equilibrium. What will happen if the volume of the container is reduced by 50% at constant temperature?
A) The forward reaction will proceed to reestablish equilibrium.
B) The reverse reaction will proceed to reestablish equilibrium.
C) No change occurs.
D) The equilibrium constant will increase.
E) The equilibrium constant will decrease.
(CH3)2CCH2(g) + H2O(g)A reaction vessel contains these compounds at equilibrium. What will happen if the volume of the container is reduced by 50% at constant temperature?
A) The forward reaction will proceed to reestablish equilibrium.
B) The reverse reaction will proceed to reestablish equilibrium.
C) No change occurs.
D) The equilibrium constant will increase.
E) The equilibrium constant will decrease.
Question
Stearic acid, nature's most common fatty acid, dimerizes when dissolved in hexane: 2C17H35COOH 
(C17H35COOH)2 ΔH°rxn = -172 kJ
The equilibrium constant for this reaction at 28°C is 2900. Estimate the equilibrium constant at 38°C.
A) 4.7 × 105
B) 2.6 × 104
C) 1.9 × 103
D) 3.2 × 102
E) 18
(C17H35COOH)2 ΔH°rxn = -172 kJThe equilibrium constant for this reaction at 28°C is 2900. Estimate the equilibrium constant at 38°C.
A) 4.7 × 105
B) 2.6 × 104
C) 1.9 × 103
D) 3.2 × 102
E) 18
Question
The reaction of nitric oxide to form dinitrogen oxide and nitrogen dioxide is exothermic. 3NO(g) 
N2O(g) + NO2(g) + heat
What effect will be seen if the temperature of the system at equilibrium is raised by 25°C?
A) The partial pressure of NO will increase.
B) The partial pressure of NO will decrease.
C) The partial pressure of NO2 will increase.
D) The partial pressures of NO and N2O will increase.
E) All three partial pressures will increase.
N2O(g) + NO2(g) + heatWhat effect will be seen if the temperature of the system at equilibrium is raised by 25°C?
A) The partial pressure of NO will increase.
B) The partial pressure of NO will decrease.
C) The partial pressure of NO2 will increase.
D) The partial pressures of NO and N2O will increase.
E) All three partial pressures will increase.
Question
The following reaction is at equilibrium at a pressure of 1 atm, in a closed container. NaOH(s) + CO2(g) 
NaHCO3(s) ΔH°rxn < 0
Which, if any, of the following actions will decrease the concentration of CO2 gas present at equilibrium?
A) adding N2 gas to double the pressure
B) adding more solid NaOH
C) increasing the volume of the container
D) lowering the temperature
E) None of these choices are correct.
NaHCO3(s) ΔH°rxn < 0Which, if any, of the following actions will decrease the concentration of CO2 gas present at equilibrium?
A) adding N2 gas to double the pressure
B) adding more solid NaOH
C) increasing the volume of the container
D) lowering the temperature
E) None of these choices are correct.
Question
Ethane can be formed by reacting acetylene with hydrogen. C2H2(g) + 2H2(g) 
C2H6(g) ΔH°rxn = -311 kJ
Under which reaction conditions would you expect to have the greatest equilibrium yield of ethane?
A) high temperature, high pressure
B) low temperature, high pressure
C) high temperature, low pressure
D) low temperature, low pressure
E) None of these choices are correct.
C2H6(g) ΔH°rxn = -311 kJUnder which reaction conditions would you expect to have the greatest equilibrium yield of ethane?
A) high temperature, high pressure
B) low temperature, high pressure
C) high temperature, low pressure
D) low temperature, low pressure
E) None of these choices are correct.
Question
A container was charged with hydrogen, nitrogen, and ammonia gases at 120°C and the system was allowed to reach equilibrium. What will happen if the volume of the container is increased at constant temperature? 3H2(g) + N2(g) 
2NH3(g)
A) There will be no effect.
B) More ammonia will be produced at the expense of hydrogen and nitrogen.
C) Hydrogen and nitrogen will be produced at the expense of ammonia.
D) The equilibrium constant will increase.
E) The equilibrium constant will decrease.
2NH3(g)A) There will be no effect.
B) More ammonia will be produced at the expense of hydrogen and nitrogen.
C) Hydrogen and nitrogen will be produced at the expense of ammonia.
D) The equilibrium constant will increase.
E) The equilibrium constant will decrease.
Question
The reaction system CS2(g) + 4H2(g) 
CH4(g) + 2H2S(g)
Is at equilibrium. Which of the following statements describes the behavior of the system if the partial pressure of carbon disulfide is reduced?
A) As equilibrium is reestablished, the partial pressure of carbon disulfide increases.
B) As equilibrium is reestablished, the partial pressure of hydrogen decreases.
C) As equilibrium is reestablished, the partial pressure of methane, CH4, increases.
D) As equilibrium is reestablished, the partial pressures of hydrogen and hydrogen sulfide decrease.
E) As equilibrium is reestablished, all the partial pressures will increase.
CH4(g) + 2H2S(g)Is at equilibrium. Which of the following statements describes the behavior of the system if the partial pressure of carbon disulfide is reduced?
A) As equilibrium is reestablished, the partial pressure of carbon disulfide increases.
B) As equilibrium is reestablished, the partial pressure of hydrogen decreases.
C) As equilibrium is reestablished, the partial pressure of methane, CH4, increases.
D) As equilibrium is reestablished, the partial pressures of hydrogen and hydrogen sulfide decrease.
E) As equilibrium is reestablished, all the partial pressures will increase.
Question
The following reaction is at equilibrium in a sealed container. N2(g) + 3H2(g) 
2NH3(g) ΔH°rxn < 0
Which, if any, of the following actions will increase the value of the equilibrium constant, Kc?
A) adding a catalyst
B) adding more N2
C) increasing the pressure
D) lowering the temperature
E) None of these choices are correct.
2NH3(g) ΔH°rxn < 0Which, if any, of the following actions will increase the value of the equilibrium constant, Kc?
A) adding a catalyst
B) adding more N2
C) increasing the pressure
D) lowering the temperature
E) None of these choices are correct.
Question
Magnesium carbonate dissociates to magnesium oxide and carbon dioxide at elevated temperatures. MgCO3(s) 
MgO(s) + CO2(g)
A reaction vessel contains these compounds in equilibrium at 300°C. What will happen if the volume of the container is reduced by 25% at 300°C?
A) The partial pressure of carbon dioxide present at equilibrium will increase.
B) The partial pressure of carbon dioxide present at equilibrium will decrease.
C) The partial pressure of carbon dioxide at equilibrium will be unchanged.
D) The equilibrium constant will have to decrease to compensate for the decrease in volume.
E) More information is needed in order to make a valid judgment.
MgO(s) + CO2(g)A reaction vessel contains these compounds in equilibrium at 300°C. What will happen if the volume of the container is reduced by 25% at 300°C?
A) The partial pressure of carbon dioxide present at equilibrium will increase.
B) The partial pressure of carbon dioxide present at equilibrium will decrease.
C) The partial pressure of carbon dioxide at equilibrium will be unchanged.
D) The equilibrium constant will have to decrease to compensate for the decrease in volume.
E) More information is needed in order to make a valid judgment.
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Deck 17: Equilibrium the Extent of Chemical Reactions
1
What is the mass-action expression, p, for the following reaction? SbF5(g) + 4Cl2(g) SbCl3(g) + 5ClF(g)
A)
B)
C)
D)
E) None of these choices are correct.
SbCl3(g) + 5ClF(g)A)
B)
C)
D)
E) None of these choices are correct.
2
What is the mass-action expression, c, for the following chemical reaction? PbO(s) + CO(g) Pb(l) + CO2(g)
A)
B)
C)
D)
E) None of these choices are correct.
c, for the following chemical reaction? PbO(s) + CO(g) Pb(l) + CO2(g)A)
B)
C)
D)
E) None of these choices are correct.
3
A chemical reaction has an equilibrium constant of 2 × 106. If this reaction is at equilibrium, select the one correct conclusion that can be made about the reaction.
A) The forward and back reactions have stopped.
B) The limiting reactant has been used up.
C) The forward and reverse rate constants are equal.
D) The forward and reverse reaction rates are equal.
E) None of these choices are correct.
A) The forward and back reactions have stopped.
B) The limiting reactant has been used up.
C) The forward and reverse rate constants are equal.
D) The forward and reverse reaction rates are equal.
E) None of these choices are correct.
The forward and reverse reaction rates are equal.
4
Write the mass-action expression, c, for the following chemical reaction. 3ClO2-(aq) 2ClO3-(aq) + Cl-(aq)
A)
B)
C)
D)
E)
A)
B)
C)
D)
E)
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5
An equilibrium is established in which both the forward (fwd) and the reverse (rev) reactions are elementary. If the equilibrium constant Kc = 1.6 × 10-2 and the rate constant kfwd = 8.0 × 10-7 s-1 what is the value of krev?
A) 1.3 × 10-8 s-1
B) 7.8 × 107 s-1
C) 2 × 104 s-1
D) 5.0 × 10-5 s-1
E) None of these choices are correct.
A) 1.3 × 10-8 s-1
B) 7.8 × 107 s-1
C) 2 × 104 s-1
D) 5.0 × 10-5 s-1
E) None of these choices are correct.
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6
Write the mass-action expression, c, for the following chemical reaction. Zn(s) + 2Ag+(aq) Zn2+(aq) + 2Ag(s)
A)
B)
C)
D)
E)
c, for the following chemical reaction. Zn(s) + 2Ag+(aq) Zn2+(aq) + 2Ag(s)A)
B)
C)
D)
E)
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7
In order to write the correct mass-action expression for a reaction one must
A) know the kinetic rate law for the reaction.
B) know the mechanism for the reaction.
C) have a properly balanced chemical equation.
D) have values for the concentrations of the reactants.
E) know the limiting reactant.
A) know the kinetic rate law for the reaction.
B) know the mechanism for the reaction.
C) have a properly balanced chemical equation.
D) have values for the concentrations of the reactants.
E) know the limiting reactant.
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8
Write the mass-action expression,
c, for the following chemical reaction equation.
2C6H6(g) + 15O2(g) 12CO2(g) + 6H2O(g)
A)
B)
C)
D)
E)
c, for the following chemical reaction equation.
2C6H6(g) + 15O2(g)
12CO2(g) + 6H2O(g)A)
B)
C)
D)
E)
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9
The reaction quotient, c, for a reaction has a value of 75 while the equilibrium constant, Kc, has a value of 195. Which of the following statements is accurate?
A) The reaction must proceed to the left to establish equilibrium.
B) The reaction must proceed to the right to establish equilibrium.
C) The concentrations of the products will be much smaller than the concentrations of the reactants when the system is at equilibrium.
D) The concentrations of the products will be about the same as the concentrations of the reactants when the system is at equilibrium.
E) None of these choices are correct.
c, for a reaction has a value of 75 while the equilibrium constant, Kc, has a value of 195. Which of the following statements is accurate?A) The reaction must proceed to the left to establish equilibrium.
B) The reaction must proceed to the right to establish equilibrium.
C) The concentrations of the products will be much smaller than the concentrations of the reactants when the system is at equilibrium.
D) The concentrations of the products will be about the same as the concentrations of the reactants when the system is at equilibrium.
E) None of these choices are correct.
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10
Carbon monoxide and chlorine combine in an equilibrium reaction to produce the highly toxic product, phosgene (COCl2) CO(g) + Cl2(g) COCl2(g)
If the equilibrium constant for this reaction is Kc = 248, predict, if possible, what will happen when the reactants and product are combined with the concentrations shown.
[CO] = [Cl2] = 0.010 M; [COCl2] = 0.070 M
A) The reaction will proceed to the right.
B) The reaction will proceed to the left.
C) The reaction is at equilibrium, and no change in concentrations will occur.
D) The container volume needs to be specified before a prediction can be made.
E) The temperature needs to be specified before a prediction can be made.
COCl2(g)If the equilibrium constant for this reaction is Kc = 248, predict, if possible, what will happen when the reactants and product are combined with the concentrations shown.
[CO] = [Cl2] = 0.010 M; [COCl2] = 0.070 M
A) The reaction will proceed to the right.
B) The reaction will proceed to the left.
C) The reaction is at equilibrium, and no change in concentrations will occur.
D) The container volume needs to be specified before a prediction can be made.
E) The temperature needs to be specified before a prediction can be made.
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11
The two equilibrium constants for the same reaction, Kc and Kp, will always equal one another when
A) all of the reactants and products are gases.
B) in the reaction equation, the number of moles of gaseous products equals the number of moles of gaseous reactants.
C) in the reaction equation, the number of moles of gaseous products is greater than the number of moles of gaseous reactants.
D) in the reaction equation, the number of moles of gaseous products is smaller than the number of moles of gaseous reactants.
E) in the reaction equation, the total number of moles of reactants equals that of the products.
A) all of the reactants and products are gases.
B) in the reaction equation, the number of moles of gaseous products equals the number of moles of gaseous reactants.
C) in the reaction equation, the number of moles of gaseous products is greater than the number of moles of gaseous reactants.
D) in the reaction equation, the number of moles of gaseous products is smaller than the number of moles of gaseous reactants.
E) in the reaction equation, the total number of moles of reactants equals that of the products.
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12
Which of the following has an effect on the magnitude of the equilibrium constant?
A) removing products as they are formed
B) adding more of a reactant
C) adding a catalyst
D) increasing the pressure, in a gas-phase reaction
E) change in temperature
A) removing products as they are formed
B) adding more of a reactant
C) adding a catalyst
D) increasing the pressure, in a gas-phase reaction
E) change in temperature
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13
Write the mass-action expression, c, for the following chemical reaction. 2Cu2+(aq) + 4I-(aq) 2CuI(s) + I2(aq)
A)
B)
C)
D)
E)
2CuI(s) + I2(aq)A)
B)
C)
D)
E)
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14
What is the mass-action expression, c, for the following chemical reaction? Cu2+(aq) + 4NH3(aq) Cu(NH3)42+(aq)
A)
B)
C)
D)
E) None of these choices are correct.
c, for the following chemical reaction? Cu2+(aq) + 4NH3(aq) Cu(NH3)42+(aq)A)
B)
C)
D)
E) None of these choices are correct.
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15
When a chemical system is at equilibrium,
A) the concentrations of the reactants are equal to the concentrations of the products.
B) the concentrations of the reactants and products have reached constant values.
C) the forward and reverse reactions have stopped.
D) the reaction quotient, , has reached a maximum.
E) the reaction quotient, , has reached a minimum.
A) the concentrations of the reactants are equal to the concentrations of the products.
B) the concentrations of the reactants and products have reached constant values.
C) the forward and reverse reactions have stopped.
D) the reaction quotient,
, has reached a maximum.E) the reaction quotient,
, has reached a minimum. Unlock Deck
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16
The reaction quotient for a gas phase reaction has a value of 2000. If the number of moles of reactants in the reaction equation is equal to that of the products, which of the following statements is definitely true?
A) The reaction must proceed to the left to establish equilibrium.
B) The reaction must proceed to the right to establish equilibrium.
C) When the system is at equilibrium, the concentrations of the products will be much larger than the concentrations of the reactants.
D) The concentrations of the products are generally larger than the concentrations of the reactants.
E) None of these choices are correct.
A) The reaction must proceed to the left to establish equilibrium.
B) The reaction must proceed to the right to establish equilibrium.
C) When the system is at equilibrium, the concentrations of the products will be much larger than the concentrations of the reactants.
D) The concentrations of the products are generally larger than the concentrations of the reactants.
E) None of these choices are correct.
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17
Carbon monoxide and chlorine combine in an equilibrium reaction to produce the highly toxic product, phosgene (COCl2) CO(g) + Cl2(g) COCl2(g)
If the equilibrium constant for this reaction is Kc = 248, predict, if possible, what will happen when the reactants and product are combined with the concentrations shown.
[CO] = [Cl2] = 0.0200 M; [COCl2] = 0.0992 M
A) The reaction will proceed to the right.
B) The reaction will proceed to the left.
C) The reaction is at equilibrium, and no change in concentrations will occur.
D) The container volume needs to be specified before a prediction can be made.
E) The temperature needs to be specified before a prediction can be made.
COCl2(g)If the equilibrium constant for this reaction is Kc = 248, predict, if possible, what will happen when the reactants and product are combined with the concentrations shown.
[CO] = [Cl2] = 0.0200 M; [COCl2] = 0.0992 M
A) The reaction will proceed to the right.
B) The reaction will proceed to the left.
C) The reaction is at equilibrium, and no change in concentrations will occur.
D) The container volume needs to be specified before a prediction can be made.
E) The temperature needs to be specified before a prediction can be made.
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18
Write the mass-action expression, c, for the following chemical reaction. Fe3+(aq) + 3OH-(aq) Fe(OH)3(s)
A)
B)
C)
D)
E)
c, for the following chemical reaction. Fe3+(aq) + 3OH-(aq) Fe(OH)3(s)A)
B)
C)
D)
E)
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19
Consider the equilibrium reaction shown below. B2(g) 2B(g)
If the rate constants are: kfwd = 7.00 × 10-5s-1 and krev = 2.00 × 10-5 L mol-1 s-1, what is the value of Kc under these conditions?
A) 1.75 × 105
B) 3.50
C) 0.286
D) 5.71 × 10-6
E) 1.40 × 10-10
2B(g)If the rate constants are: kfwd = 7.00 × 10-5s-1 and krev = 2.00 × 10-5 L mol-1 s-1, what is the value of Kc under these conditions?
A) 1.75 × 105
B) 3.50
C) 0.286
D) 5.71 × 10-6
E) 1.40 × 10-10
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20
Write the mass-action expression, c, for the following chemical reaction. NO(g) + ½Br2(g) NOBr(g)
A)
B)
C)
D)
E)
c, for the following chemical reaction. NO(g) + ½Br2(g) NOBr(g)A)
B)
C)
D)
E)
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21
Consider the following two equilibria and their respective equilibrium constants: (1) NO(g) + ½O2(g) NO2(g)
(2) 2NO2(g) 2NO(g) + O2(g)
Which one of the following is the correct relationship between the equilibrium constants K1 and K2?
A) K2 = 2/K1
B) K2 = (1/K1)2
C) K2 = -K1/2
D) K2 = 1/(2K1)
E) K2 = 1/(2K1)2
NO2(g)(2) 2NO2(g)
2NO(g) + O2(g)Which one of the following is the correct relationship between the equilibrium constants K1 and K2?
A) K2 = 2/K1
B) K2 = (1/K1)2
C) K2 = -K1/2
D) K2 = 1/(2K1)
E) K2 = 1/(2K1)2
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22
Write the mass-action expression, c, for the following chemical reaction. Sn2+(aq) + ½O2(g) + 3H2O(l) SnO2(s) + 2H3O+(aq)
A)
B)
C)
D)
E) None of these choices are correct.
c, for the following chemical reaction. Sn2+(aq) + ½O2(g) + 3H2O(l) SnO2(s) + 2H3O+(aq)A)
B)
C)
D)
E) None of these choices are correct.
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23
The equilibrium constant for reaction (1) below is 276. Under the same conditions, what is the equilibrium constant of reaction (2)? (1) ½X2(g) + ½Y2(g) XY(g)
(2) 2XY(g) X2(g) + Y2(g)
A) 6.02 × 10-2
B) 7.25 × 10-3
C) 3.62 × 10-3
D) 1.31 × 10-5
E) None of these choices are correct.
XY(g)(2) 2XY(g)
X2(g) + Y2(g)A) 6.02 × 10-2
B) 7.25 × 10-3
C) 3.62 × 10-3
D) 1.31 × 10-5
E) None of these choices are correct.
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24
The equilibrium constant, Kc, for the decomposition of COBr2 COBr2(g) CO(g) + Br2(g)
Is 0.190. What is Kc for the following reaction?
2CO(g) + 2Br2(g) 2COBr2(g)
A) 0.0361
B) 2.63
C) 5.62
D) 10.5
E) 27.7
CO(g) + Br2(g)Is 0.190. What is Kc for the following reaction?
2CO(g) + 2Br2(g)
2COBr2(g)A) 0.0361
B) 2.63
C) 5.62
D) 10.5
E) 27.7
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25
The equilibrium constant, Kp, for the reaction H2(g) + I2(g) 2HI(g)
Is 55.2 at 425°C. A rigid cylinder at that temperature contains 0.127 atm of hydrogen, 0.134 atm of iodine, and 1.055 atm of hydrogen iodide. Is the system at equilibrium?
A) Yes.
B) No, the forward reaction must proceed to establish equilibrium.
C) No, the reverse reaction must proceed to establish equilibrium.
D) Need to know the volume of the container before deciding.
E) Need to know the starting concentrations of all substances before deciding.
2HI(g)Is 55.2 at 425°C. A rigid cylinder at that temperature contains 0.127 atm of hydrogen, 0.134 atm of iodine, and 1.055 atm of hydrogen iodide. Is the system at equilibrium?
A) Yes.
B) No, the forward reaction must proceed to establish equilibrium.
C) No, the reverse reaction must proceed to establish equilibrium.
D) Need to know the volume of the container before deciding.
E) Need to know the starting concentrations of all substances before deciding.
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26
What is the mass-action expression, c, for the following chemical reaction? 4H3O+(aq) + 2Cl-(aq) + MnO2(s) Mn2+(aq) + 6H2O(l) + Cl2(g)
A)
B)
C)
D)
E) None of these choices are correct.
c, for the following chemical reaction? 4H3O+(aq) + 2Cl-(aq) + MnO2(s) Mn2+(aq) + 6H2O(l) + Cl2(g)A)
B)
C)
D)
E) None of these choices are correct.
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27
The reaction of nitrogen with oxygen to form nitrogen monoxide can be represented by the following equation. N2(g) + O2(g) 2NO(g)
At 2000°C, the equilibrium constant, Kc, has a value of 4.10 × 10-4. What is the value of Kp?
A) 2.17 × 10-8
B) 4.10 × 10-4
C) 7.65 × 10-2
D) 7.75
E) None of these choices are correct.
2NO(g)At 2000°C, the equilibrium constant, Kc, has a value of 4.10 × 10-4. What is the value of Kp?
A) 2.17 × 10-8
B) 4.10 × 10-4
C) 7.65 × 10-2
D) 7.75
E) None of these choices are correct.
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28
Write the mass-action expression, c, for the following chemical reaction. MgO(s) + SO2(g) + ½O2(g) MgSO4(s)
A)
B)
C)
D)
E) None of these choices are correct.
c, for the following chemical reaction. MgO(s) + SO2(g) + ½O2(g) MgSO4(s)A)
B)
C)
D)
E) None of these choices are correct.
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29
Nitrogen dioxide decomposes according to the reaction 2NO2(g) 2NO(g) + O2(g)
Where Kp = 4.48 × 10-13 at 25°C. What is the value for Kc?
A) 1.81 × 10-16
B) 1.83 × 10-14
C) 4.48 × 10-13
D) 1.10 × 10-11
E) 1.11 × 10-9
2NO(g) + O2(g)Where Kp = 4.48 × 10-13 at 25°C. What is the value for Kc?
A) 1.81 × 10-16
B) 1.83 × 10-14
C) 4.48 × 10-13
D) 1.10 × 10-11
E) 1.11 × 10-9
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30
Consider the equilibrium reaction: H2(g) + Br2(g) 2HBr(g) Which of the following correctly describes the relationship between Kc and Kp for the reaction?
A) Kp = Kc
B) Kp = (RT)Kc
C) Kp = (RT)2Kc
D) Kp = Kc / RT
E) Kp = Kc / (RT)2
2HBr(g) Which of the following correctly describes the relationship between Kc and Kp for the reaction?A) Kp = Kc
B) Kp = (RT)Kc
C) Kp = (RT)2Kc
D) Kp = Kc / RT
E) Kp = Kc / (RT)2
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31
About half of the sodium carbonate produced is used in making glass products because it lowers the melting point of sand, the major component of glass. When sodium carbonate is added to water it hydrolyses according to the following reactions. CO32-(aq) + H2O(l) HCO3-(aq) + OH-(aq) K1
HCO3(aq) + H2O(l) H2CO3(aq) + OH-(aq) K2
These can be combined to yield
CO32-(aq) + 2H2O(l) H2CO3(aq) + 2OH-(aq) K3
What is the value of K3?
A) K1 × K2
B) K1 ÷ K2
C) K1 + K2
D) K1 - K2
E) (K1K2)2
HCO3-(aq) + OH-(aq) K1HCO3(aq) + H2O(l)
H2CO3(aq) + OH-(aq) K2These can be combined to yield
CO32-(aq) + 2H2O(l)
H2CO3(aq) + 2OH-(aq) K3What is the value of K3?
A) K1 × K2
B) K1 ÷ K2
C) K1 + K2
D) K1 - K2
E) (K1K2)2
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32
N2(g) + O2(g) 2NO(g) Kc = 4.8 × 10-31 2NOBr(g) 2NO(g) + Br2(g) Kc = 0.50
Given the above equilibrium constant data at 25°C, what is the value of Kc at this temperature for the reaction
2NOBr(g) N2(g) + O2(g) + Br2(g)?
A) 2.4 × 10-31
B) 9.6 × 10-31
C) 1.0 × 1030
D) 4.2 × 1030
E) None of these choices are correct.
2NO(g) Kc = 4.8 × 10-31 2NOBr(g) 2NO(g) + Br2(g) Kc = 0.50Given the above equilibrium constant data at 25°C, what is the value of Kc at this temperature for the reaction
2NOBr(g)
N2(g) + O2(g) + Br2(g)?A) 2.4 × 10-31
B) 9.6 × 10-31
C) 1.0 × 1030
D) 4.2 × 1030
E) None of these choices are correct.
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33
The equilibrium constant for the reaction of bromine with chlorine to form bromine monochloride is 58.0 at a certain temperature. Br2(g) + Cl2(g) 2BrCl(g)
What is the equilibrium constant for the following reaction?
BrCl(g) ½Br2(g) + ½Cl2(g)
A) 2.97 × 10-4
B) 1.72 × 10-2
C) 3.45 × 10-2
D) 1.31 × 10-1
E) > 1.00
2BrCl(g)What is the equilibrium constant for the following reaction?
BrCl(g)
½Br2(g) + ½Cl2(g)A) 2.97 × 10-4
B) 1.72 × 10-2
C) 3.45 × 10-2
D) 1.31 × 10-1
E) > 1.00
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34
The equilibrium constant, Kp, has a value of 6.5 × 10-4 at 308 K for the reaction of nitrogen monoxide with chlorine. 2NO(g) + Cl2(g) 2NOCl(g)
What is the value of Kc?
A) 2.5 × 10-7
B) 6.5 × 10-4
C) 1.6 × 10-2
D) 1.7
E) None of these choices are correct.
2NOCl(g)What is the value of Kc?
A) 2.5 × 10-7
B) 6.5 × 10-4
C) 1.6 × 10-2
D) 1.7
E) None of these choices are correct.
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35
H2SO3(aq) HSO3(aq) + H+(aq) Kc = 1.4 × 10-2 H2SO3(aq) SO32-(aq) + 2H+(aq) Kc = 9.1 × 10-10
Given the above equilibrium constant data at 25°C, what is the value of Kc at this temperature for the reaction
HSO3-(aq) SO32-(aq) + H+(aq)?
A) 6.5 ×10-8
B) 1.3 × 10-11
C) 7.8 × 1010
D) 1.5 × 107
E) None of these choices are correct.
HSO3(aq) + H+(aq) Kc = 1.4 × 10-2 H2SO3(aq) SO32-(aq) + 2H+(aq) Kc = 9.1 × 10-10Given the above equilibrium constant data at 25°C, what is the value of Kc at this temperature for the reaction
HSO3-(aq)
SO32-(aq) + H+(aq)?A) 6.5 ×10-8
B) 1.3 × 10-11
C) 7.8 × 1010
D) 1.5 × 107
E) None of these choices are correct.
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36
In water, the following equilibrium exists: H+(aq) + OH-(aq) H2O(l)
In pure water at 25°C, the concentration of H+ ions is 1.00 × 10-7 mol/L. Calculate the value of the equilibrium constant for the reaction as written above.
A) 1.00 × 1014
B) 1.00 × 1012
C) 1.00 × 10-14
D) 1.00 × 10-12
E) 5.55 × 1015
H2O(l)In pure water at 25°C, the concentration of H+ ions is 1.00 × 10-7 mol/L. Calculate the value of the equilibrium constant for the reaction as written above.
A) 1.00 × 1014
B) 1.00 × 1012
C) 1.00 × 10-14
D) 1.00 × 10-12
E) 5.55 × 1015
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37
Hydrogen sulfide will react with water as shown in the following reactions. H2S(g) + H2O(l) H3O+(aq) + HS-(aq) K1 = 1.0 × 10-7
HS-(aq) + H2O(l) H3O+(aq) + S2-(aq) K2 = ?
H2S(g) + 2H2O(l) 2H3O+(aq) + S2-(aq) K3 = 1.3 × 10-20
What is the value of K2?
A) 1.3 × 10-27
B) 2.3 × 10-7
C) 1.3 × 10-13
D) 7.7 × 1012
E) 7.7 × 1026
H3O+(aq) + HS-(aq) K1 = 1.0 × 10-7HS-(aq) + H2O(l)
H3O+(aq) + S2-(aq) K2 = ?H2S(g) + 2H2O(l)
2H3O+(aq) + S2-(aq) K3 = 1.3 × 10-20What is the value of K2?
A) 1.3 × 10-27
B) 2.3 × 10-7
C) 1.3 × 10-13
D) 7.7 × 1012
E) 7.7 × 1026
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38
Consider the equilibrium reaction: N2O4(g) 2NO2(g) Which of the following correctly describes the relationship between Kc and Kp for the reaction?
A) Kp = Kc
B) Kp = RT × Kc
C) Kp = (RT × Kc)-1
D) Kp = Kc / RT
E) Kp = RT / Kc
2NO2(g) Which of the following correctly describes the relationship between Kc and Kp for the reaction?A) Kp = Kc
B) Kp = RT × Kc
C) Kp = (RT × Kc)-1
D) Kp = Kc / RT
E) Kp = RT / Kc
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39
Consider the reactions of cadmium with the thiosulfate anion. Cd2+(aq) + S2O32-(aq) Cd(S2O3)(aq) K1 = 8.3 × 103
Cd(S2O3)(aq) + S2O32-(aq) Cd(S2O3)22-(aq) K2 = 2.5 × 102
What is the value for the equilibrium constant for the following reaction?
Cd2+(aq) + 2S2O32-(aq) Cd(S2O3)22-(aq)
A) 0.030
B) 33
C) 8.1 × 103
D) 8.6 × 103
E) 2.1 × 106
Cd(S2O3)(aq) K1 = 8.3 × 103Cd(S2O3)(aq) + S2O32-(aq)
Cd(S2O3)22-(aq) K2 = 2.5 × 102What is the value for the equilibrium constant for the following reaction?
Cd2+(aq) + 2S2O32-(aq)
Cd(S2O3)22-(aq)A) 0.030
B) 33
C) 8.1 × 103
D) 8.6 × 103
E) 2.1 × 106
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40
At 500°C the equilibrium constant, Kp, is 4.00 × 10-4 for the equilibrium: 2HCN(g) H2(g) + C2N2(g)
What is Kp for the following reaction?
H2(g) + C2N2(g) 2HCN(g)
A) 2.00 × 10-4
B) -4.00 × 10-4
C) 1.25 × 103
D) 2.50 × 103
E) 4.00 × 104
H2(g) + C2N2(g)What is Kp for the following reaction?
H2(g) + C2N2(g)
2HCN(g)A) 2.00 × 10-4
B) -4.00 × 10-4
C) 1.25 × 103
D) 2.50 × 103
E) 4.00 × 104
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41
10.0 mL of a 0.100 mol L-1 solution of a metal ion M2+ is mixed with 10.0 mL of a 0.100 mol L-1 solution of a substance L. The following equilibrium is established: M2+(aq) + 2L(aq) ML22+(aq)
At equilibrium the concentration of L is found to be 0.0100 mol L-1. What is the equilibrium concentration of ML22+, in mol L-1?
A) 0.100 mol L-1
B) 0.050 mol L-1
C) 0.025 mol L-1
D) 0.0200 mol L-1
E) 0.0100 mol L-1
ML22+(aq)At equilibrium the concentration of L is found to be 0.0100 mol L-1. What is the equilibrium concentration of ML22+, in mol L-1?
A) 0.100 mol L-1
B) 0.050 mol L-1
C) 0.025 mol L-1
D) 0.0200 mol L-1
E) 0.0100 mol L-1
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42
Nitric oxide and bromine were allowed to react in a sealed container. When equilibrium was reached PNO = 0.526 atm, = 1.59 atm, and PNOBr = 7.68 atm. Calculate Kp for the reaction.
2NO(g) + Br2(g) 2NOBr(g)
A) 7.45 × 10-3
B) 0.109
C) 9.18
D) 91.8
E) 134
= 1.59 atm, and PNOBr = 7.68 atm. Calculate Kp for the reaction.2NO(g) + Br2(g)
2NOBr(g)A) 7.45 × 10-3
B) 0.109
C) 9.18
D) 91.8
E) 134
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43
Hydrogen iodide, HI, is formed in an equilibrium reaction when gaseous hydrogen and iodine gas are heated together. If 20.0 g of hydrogen and 20.0 g of iodine are heated, forming 10.0 g of hydrogen iodide, what mass of hydrogen remains unreacted?
A) 10.0 g hydrogen remains
B) 10.9 g hydrogen remains
C) 15.0 g hydrogen remains
D) 19.9 g hydrogen remains
E) Need to know the equilibrium constant in order to calculate the answer.
A) 10.0 g hydrogen remains
B) 10.9 g hydrogen remains
C) 15.0 g hydrogen remains
D) 19.9 g hydrogen remains
E) Need to know the equilibrium constant in order to calculate the answer.
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44
At 850°C, the equilibrium constant Kp for the reaction C(s) + CO2(g) 2CO(g)
Has a value of 10.7. If the total pressure in the system at equilibrium is 1.000 atm, what is the partial pressure of carbon monoxide?
A) 0.362 atm
B) 0.489 atm
C) 0.667 atm
D) 0.915 atm
E) 0.921 atm
2CO(g)Has a value of 10.7. If the total pressure in the system at equilibrium is 1.000 atm, what is the partial pressure of carbon monoxide?
A) 0.362 atm
B) 0.489 atm
C) 0.667 atm
D) 0.915 atm
E) 0.921 atm
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45
At 25°C, the equilibrium constant Kc for the reaction 2A(aq) B(aq) + C(aq)
Is 65. If 2.50 mol of A is added to enough water to prepare 1.00 L of solution, what will the equilibrium concentration of A be?
A) 0.038 M
B) 0.14 M
C) 0.28 M
D) 1.18 M
E) 2.4 M
B(aq) + C(aq)Is 65. If 2.50 mol of A is added to enough water to prepare 1.00 L of solution, what will the equilibrium concentration of A be?
A) 0.038 M
B) 0.14 M
C) 0.28 M
D) 1.18 M
E) 2.4 M
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46
SO2 reacts with O2 to produce SO3. If 86.0 g of SO2 is placed in a reaction vessel along with excess oxygen gas, how many moles of SO2 remain when 50.0 g of SO3 have been formed?
A) 0.56 mol
B) 0.62 mol
C) 0.72 mol
D) 0.78 mol
E) 1.34 mol
A) 0.56 mol
B) 0.62 mol
C) 0.72 mol
D) 0.78 mol
E) 1.34 mol
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47
Ammonium iodide dissociates reversibly to ammonia and hydrogen iodide. NH4I(s) NH3(g) + HI(g)
At 400°C, Kp = 0.215. Calculate the partial pressure of ammonia at equilibrium when a sufficient quantity of ammonium iodide is heated to 400°C.
A) 0.103 atm
B) 0.215 atm
C) 0.232 atm
D) 0.464 atm
E) 2.00 atm
NH3(g) + HI(g)At 400°C, Kp = 0.215. Calculate the partial pressure of ammonia at equilibrium when a sufficient quantity of ammonium iodide is heated to 400°C.
A) 0.103 atm
B) 0.215 atm
C) 0.232 atm
D) 0.464 atm
E) 2.00 atm
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48
At a certain temperature the reaction CO2(g) + H2(g) CO(g) + H2O(g)2
Has Kc = 2.50. If 2.00 mol of carbon dioxide and 1.5 mol of hydrogen are placed in a 5.00 L vessel and equilibrium is established, what will be the concentration of carbon monoxide?
A) 0.091 M
B) 0.191 M
C) 0.209 M
D) 0.913 M
E) 1.05 M
CO(g) + H2O(g)2Has Kc = 2.50. If 2.00 mol of carbon dioxide and 1.5 mol of hydrogen are placed in a 5.00 L vessel and equilibrium is established, what will be the concentration of carbon monoxide?
A) 0.091 M
B) 0.191 M
C) 0.209 M
D) 0.913 M
E) 1.05 M
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49
A mixture of 0.500 mole of carbon monoxide and 0.400 mole of bromine was placed into a rigid 1.00-L container and the system was allowed to come to equilibrium. The equilibrium
Concentration of COBr2 was 0.233 M. What is the value of Kc for this reaction?
CO(g) + Br2(g) COBr2(g)
A) 5.23
B) 1.22
C) 1.165
D) 0.858
E) 0.191
Concentration of COBr2 was 0.233 M. What is the value of Kc for this reaction?
CO(g) + Br2(g)
COBr2(g)A) 5.23
B) 1.22
C) 1.165
D) 0.858
E) 0.191
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50
The equilibrium constant, Kp, for the reaction CO(g) + H2O(g) CO2(g) + H2(g)
At 986°C is 0.63. A rigid cylinder at that temperature contains 1.2 atm of carbon monoxide, 0.20 atm of water vapor, 0.30 atm of carbon dioxide, and 0.27 atm of hydrogen. Is the system at equilibrium?
A) Yes.
B) No, the forward reaction must proceed to establish equilibrium.
C) No, the reverse reaction must proceed to establish equilibrium.
D) Need to know the volume of the container before deciding.
E) Need to know the starting concentrations of all substances before deciding.
CO2(g) + H2(g)At 986°C is 0.63. A rigid cylinder at that temperature contains 1.2 atm of carbon monoxide, 0.20 atm of water vapor, 0.30 atm of carbon dioxide, and 0.27 atm of hydrogen. Is the system at equilibrium?
A) Yes.
B) No, the forward reaction must proceed to establish equilibrium.
C) No, the reverse reaction must proceed to establish equilibrium.
D) Need to know the volume of the container before deciding.
E) Need to know the starting concentrations of all substances before deciding.
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51
The equilibrium constant Kc for the reaction PCl3(g) + Cl2(g) PCl5(g)
Is 49 at 230°C. If 0.70 mol of PCl3 is added to 0.70 mol of Cl2 in a 1.00-L reaction vessel at 230°C, what is the concentration of PCl3 when equilibrium has been established?
A) 0.049 M
B) 0.11 M
C) 0.30 M
D) 0.59 M
E) 0.83 M
PCl5(g)Is 49 at 230°C. If 0.70 mol of PCl3 is added to 0.70 mol of Cl2 in a 1.00-L reaction vessel at 230°C, what is the concentration of PCl3 when equilibrium has been established?
A) 0.049 M
B) 0.11 M
C) 0.30 M
D) 0.59 M
E) 0.83 M
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52
At high temperatures, carbon reacts with O2 to produce CO as follows: C(s) + O2(g) 2CO(g).
When 0.350 mol of O2 and excess carbon were placed in a 5.00-L container and heated, the equilibrium concentration of CO was found to be 0.060 M. What is the equilibrium constant, Kc, for this reaction?
A) 0.010
B) 0.072
C) 0.090
D) 0.17
E) 1.2
2CO(g).When 0.350 mol of O2 and excess carbon were placed in a 5.00-L container and heated, the equilibrium concentration of CO was found to be 0.060 M. What is the equilibrium constant, Kc, for this reaction?
A) 0.010
B) 0.072
C) 0.090
D) 0.17
E) 1.2
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53
The equilibrium constant Kc for the reaction A(g) + B(g) C(g)
Is 0.76 at 150°C. If 0.800 mol of A is added to 0.600 mol of B in a 1.00-L container at 150°C, what will be the equilibrium concentration of C?
A) 0.19 M
B) 0.29 M
C) 0.36 M
D) 0.41 M
E) 0.51 M
C(g)Is 0.76 at 150°C. If 0.800 mol of A is added to 0.600 mol of B in a 1.00-L container at 150°C, what will be the equilibrium concentration of C?
A) 0.19 M
B) 0.29 M
C) 0.36 M
D) 0.41 M
E) 0.51 M
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54
Compounds A, B, and C react according to the following equation. 3A(g) + 2B(g) 2C(g)
At 100°C a mixture of these gases at equilibrium showed that [A] = 0.855 M, [B] = 1.23 M, and [C] = 1.75 M. What is the value of Kc for this reaction?
A) 0.309
B) 0.601
C) 1.66
D) 3.24
E) > 10
2C(g)At 100°C a mixture of these gases at equilibrium showed that [A] = 0.855 M, [B] = 1.23 M, and [C] = 1.75 M. What is the value of Kc for this reaction?
A) 0.309
B) 0.601
C) 1.66
D) 3.24
E) > 10
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55
The reaction system POCl3(g) POCl(g) + Cl2(g)
Is at equilibrium. Which of the following statements describes the behavior of the system if POCl is added to the container?
A) The forward reaction will proceed to establish equilibrium.
B) The reverse reaction will proceed to establish equilibrium.
C) The partial pressures of POCl3 and POCl will remain steady while the partial pressure of chlorine increases.
D) The partial pressure of chlorine remains steady while the partial pressures of POCl3 and POCl increase.
E) The partial pressure of chlorine will increase while the partial pressure of POCl decreases.
POCl(g) + Cl2(g)Is at equilibrium. Which of the following statements describes the behavior of the system if POCl is added to the container?
A) The forward reaction will proceed to establish equilibrium.
B) The reverse reaction will proceed to establish equilibrium.
C) The partial pressures of POCl3 and POCl will remain steady while the partial pressure of chlorine increases.
D) The partial pressure of chlorine remains steady while the partial pressures of POCl3 and POCl increase.
E) The partial pressure of chlorine will increase while the partial pressure of POCl decreases.
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56
The following reaction, in CCl4 solvent, has been studied at 25°C. 2BrCl Br2 + Cl2
The equilibrium constant Kc is known to be 0.141. If the initial concentration of chlorine is 0.0300 M and of bromine monochloride is 0.0200 M, what is the equilibrium concentration of bromine?
A) 1.35 × 10-3 M
B) 2.70 × 10-3 M
C) 8.82 × 10-3 M
D) 9.70 × 10-2 M
E) None of these choices are correct.
Br2 + Cl2The equilibrium constant Kc is known to be 0.141. If the initial concentration of chlorine is 0.0300 M and of bromine monochloride is 0.0200 M, what is the equilibrium concentration of bromine?
A) 1.35 × 10-3 M
B) 2.70 × 10-3 M
C) 8.82 × 10-3 M
D) 9.70 × 10-2 M
E) None of these choices are correct.
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57
At 25°C, the equilibrium constant Kc for the reaction 2A(g) B(g) + C(g)
Is 0.035. A mixture of 8.00 moles of B and 12.00 moles of C in a 20.0 L container is allowed to come to equilibrium. What is the equilibrium concentration of A?
A) < 0.100 M
B) 0.339 M
C) 0.678 M
D) 6.78 M
E) 13.56 M
B(g) + C(g)Is 0.035. A mixture of 8.00 moles of B and 12.00 moles of C in a 20.0 L container is allowed to come to equilibrium. What is the equilibrium concentration of A?
A) < 0.100 M
B) 0.339 M
C) 0.678 M
D) 6.78 M
E) 13.56 M
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58
Consider the reversible reaction: 2NO2(g) N2O4(g) If the concentrations of both NO2 and N2O4 are 0.016 mol L-1, what is the value of
c?
A) 0.016
B) 0.50
C) 1.0
D) 2.0
E) 63
N2O4(g) If the concentrations of both NO2 and N2O4 are 0.016 mol L-1, what is the value of c?
A) 0.016
B) 0.50
C) 1.0
D) 2.0
E) 63
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59
A mixture of 0.600 mol of bromine and 1.600 mol of iodine is placed into a rigid 1.000-L container at 350°C. Br2(g) + I2(g) 2IBr(g)
When the mixture has come to equilibrium, the concentration of iodine monobromide is 1.190 M. What is the equilibrium constant for this reaction at 350°C?
A) 3.55 × 10-3
B) 1.24
C) 1.47
D) 282
E) 325
2IBr(g)When the mixture has come to equilibrium, the concentration of iodine monobromide is 1.190 M. What is the equilibrium constant for this reaction at 350°C?
A) 3.55 × 10-3
B) 1.24
C) 1.47
D) 282
E) 325
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60
Nitric oxide is formed in automobile exhaust when nitrogen and oxygen in air react at high temperatures. N2(g) + O2(g) 2NO(g)
The equilibrium constant Kp for the reaction is 0.0025 at 2127°C. If a container is charged with 8.00 atm of nitrogen and 5.00 atm of oxygen and the mixture is allowed to reach equilibrium, what will be the equilibrium partial pressure of nitrogen?
A) 0.16 atm
B) 0.31 atm
C) 3.1 atm
D) 7.7 atm
E) 7.8 atm
2NO(g)The equilibrium constant Kp for the reaction is 0.0025 at 2127°C. If a container is charged with 8.00 atm of nitrogen and 5.00 atm of oxygen and the mixture is allowed to reach equilibrium, what will be the equilibrium partial pressure of nitrogen?
A) 0.16 atm
B) 0.31 atm
C) 3.1 atm
D) 7.7 atm
E) 7.8 atm
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61
The reaction system CS2(g) + 4H2(g) CH4(g) + 2H2S(g)
Is at equilibrium. Which of the following statements describes the behavior of the system if the partial pressure of hydrogen is doubled?
A) As equilibrium is reestablished, the partial pressure of carbon disulfide increases.
B) As equilibrium is reestablished, the partial pressure of methane, CH4, decreases.
C) As equilibrium is reestablished, the partial pressure of hydrogen decreases.
D) As equilibrium is reestablished, the partial pressure of hydrogen sulfide decreases.
E) As equilibrium is reestablished, all the partial pressures will decrease.
CH4(g) + 2H2S(g)Is at equilibrium. Which of the following statements describes the behavior of the system if the partial pressure of hydrogen is doubled?
A) As equilibrium is reestablished, the partial pressure of carbon disulfide increases.
B) As equilibrium is reestablished, the partial pressure of methane, CH4, decreases.
C) As equilibrium is reestablished, the partial pressure of hydrogen decreases.
D) As equilibrium is reestablished, the partial pressure of hydrogen sulfide decreases.
E) As equilibrium is reestablished, all the partial pressures will decrease.
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62
The following reaction is at equilibrium at one atmosphere, in a closed container. NaOH(s) + CO2(g) NaHCO3(s)
Which, if any, of the following actions will decrease the total amount of CO2 gas present at equilibrium?
A) adding N2 gas to double the pressure
B) adding more solid NaOH
C) decreasing the volume of the container
D) removing half of the solid NaHCO3
E) None of these choices are correct.
NaHCO3(s)Which, if any, of the following actions will decrease the total amount of CO2 gas present at equilibrium?
A) adding N2 gas to double the pressure
B) adding more solid NaOH
C) decreasing the volume of the container
D) removing half of the solid NaHCO3
E) None of these choices are correct.
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63
Nitrogen dioxide can dissociate to nitric oxide and oxygen. 2NO2(g) 2NO(g) + O2(g) ΔH°rxn = +114 kJ
Under which reaction conditions would you expect to produce the largest amount of oxygen?
A) high temperature, high pressure
B) low temperature, high pressure
C) high temperature, low pressure
D) low temperature, low pressure
E) None of these choices are correct.
2NO(g) + O2(g) ΔH°rxn = +114 kJUnder which reaction conditions would you expect to produce the largest amount of oxygen?
A) high temperature, high pressure
B) low temperature, high pressure
C) high temperature, low pressure
D) low temperature, low pressure
E) None of these choices are correct.
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64
Methanol can be synthesized by combining carbon monoxide and hydrogen. CO(g) + 2H2(g) CH3OH(g) ΔH°rxn = -90.7 kJ
A reaction vessel contains these compounds at equilibrium. What effect will be seen when equilibrium is re-established after decreasing the temperature by 45°C?
A) All the partial pressures will decrease.
B) The partial pressure of methanol will decrease.
C) The partial pressures of hydrogen and methanol will decrease.
D) The partial pressure of hydrogen will increase.
E) The partial pressure of carbon monoxide will decrease.
CH3OH(g) ΔH°rxn = -90.7 kJA reaction vessel contains these compounds at equilibrium. What effect will be seen when equilibrium is re-established after decreasing the temperature by 45°C?
A) All the partial pressures will decrease.
B) The partial pressure of methanol will decrease.
C) The partial pressures of hydrogen and methanol will decrease.
D) The partial pressure of hydrogen will increase.
E) The partial pressure of carbon monoxide will decrease.
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65
Sodium hydrogen carbonate decomposes above 110°C to form sodium carbonate, water, and carbon dioxide. 2NaHCO3(s) Na2CO3(s) + H2O(g) + CO2(g)
One thousand grams of sodium hydrogen carbonate are added to a reaction vessel, the temperature is increased to 200°C, and the system comes to equilibrium. What happens in this system if another 50 g of sodium carbonate are now added?
A) The partial pressure of carbon dioxide will increase.
B) The partial pressure of carbon dioxide will decrease.
C) The partial pressure of carbon dioxide will be unchanged.
D) The amounts of all products will be greater when equilibrium is reestablished.
E) None of these choices are correct.
Na2CO3(s) + H2O(g) + CO2(g)One thousand grams of sodium hydrogen carbonate are added to a reaction vessel, the temperature is increased to 200°C, and the system comes to equilibrium. What happens in this system if another 50 g of sodium carbonate are now added?
A) The partial pressure of carbon dioxide will increase.
B) The partial pressure of carbon dioxide will decrease.
C) The partial pressure of carbon dioxide will be unchanged.
D) The amounts of all products will be greater when equilibrium is reestablished.
E) None of these choices are correct.
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66
Hydrogen sulfide can be formed in the following reaction: H2(g) + ½S2(g) H2S(g) ΔH°rxn = -92 kJ
The equilibrium constant Kp = 106 at 1023 K. Estimate the value of Kp at 1218 K.
A) 5.05
B) 18.8
C) 34.7
D) 88.9
E) 598
H2S(g) ΔH°rxn = -92 kJThe equilibrium constant Kp = 106 at 1023 K. Estimate the value of Kp at 1218 K.
A) 5.05
B) 18.8
C) 34.7
D) 88.9
E) 598
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67
The reaction system POCl3(g) POCl(g) + Cl2(g)
Is at equilibrium. Which of the following statements describes the behavior of the system if the partial pressure of chlorine is reduced by 50%?
A) POCl3 will be consumed as equilibrium is established.
B) POCl will be consumed as equilibrium is established.
C) Chlorine will be consumed as equilibrium is established.
D) The partial pressure of POCl will decrease while the partial pressure of Cl2 increases as equilibrium is established.
E) The volume will have to decrease before equilibrium can be reestablished.
POCl(g) + Cl2(g)Is at equilibrium. Which of the following statements describes the behavior of the system if the partial pressure of chlorine is reduced by 50%?
A) POCl3 will be consumed as equilibrium is established.
B) POCl will be consumed as equilibrium is established.
C) Chlorine will be consumed as equilibrium is established.
D) The partial pressure of POCl will decrease while the partial pressure of Cl2 increases as equilibrium is established.
E) The volume will have to decrease before equilibrium can be reestablished.
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68
The following reaction is at equilibrium in a closed container. CuSO4.5H2O(s) CuSO4(s) + 5H2O(g)
Which, if any, of the following actions will lead to an increase in the pressure of H2O present at equilibrium?
A) increasing the volume of the container
B) decreasing the volume of the container
C) adding a catalyst
D) removing some solid CuSO4
E) None of these choices are correct.
CuSO4(s) + 5H2O(g)Which, if any, of the following actions will lead to an increase in the pressure of H2O present at equilibrium?
A) increasing the volume of the container
B) decreasing the volume of the container
C) adding a catalyst
D) removing some solid CuSO4
E) None of these choices are correct.
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69
Methanol can be synthesized by combining carbon monoxide and hydrogen. CO(g) + 2H2(g) CH3OH(g)
A reaction vessel contains the three gases at equilibrium with a total pressure of 1.00 atm. What will happen to the partial pressure of hydrogen if enough argon is added to raise the total pressure to 1.4 atm?
A) The partial pressure of hydrogen will decrease.
B) The partial pressure of hydrogen will increase.
C) The partial pressure of hydrogen will be unchanged.
D) Kp needs to be known before a prediction can be made.
E) Both Kp and the temperature need to be known before a prediction can be made.
CH3OH(g)A reaction vessel contains the three gases at equilibrium with a total pressure of 1.00 atm. What will happen to the partial pressure of hydrogen if enough argon is added to raise the total pressure to 1.4 atm?
A) The partial pressure of hydrogen will decrease.
B) The partial pressure of hydrogen will increase.
C) The partial pressure of hydrogen will be unchanged.
D) Kp needs to be known before a prediction can be made.
E) Both Kp and the temperature need to be known before a prediction can be made.
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70
Magnesium hydroxide is used in several antacid formulations. When it is added to water it dissociates into magnesium and hydroxide ions. Mg(OH)2(s) Mg2+(aq) + 2OH-(aq)
The equilibrium constant at 25°C is 8.9 × 10-12. One hundred grams of magnesium hydroxide is added to 1.00 L of water and equilibrium is established. What happens to the solution if another 10 grams of Mg(OH)2 are now added to the mixture?
A) The hydroxide ion concentration will decrease.
B) The hydroxide ion concentration will increase.
C) The hydroxide ion concentration will be unchanged.
D) The solution will become supersaturated.
E) None of these choices are correct.
Mg2+(aq) + 2OH-(aq)The equilibrium constant at 25°C is 8.9 × 10-12. One hundred grams of magnesium hydroxide is added to 1.00 L of water and equilibrium is established. What happens to the solution if another 10 grams of Mg(OH)2 are now added to the mixture?
A) The hydroxide ion concentration will decrease.
B) The hydroxide ion concentration will increase.
C) The hydroxide ion concentration will be unchanged.
D) The solution will become supersaturated.
E) None of these choices are correct.
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71
Hydrogen bromide will dissociate into hydrogen and bromine gases. 2HBr(g) H2(g) + Br2(g) ΔH°rxn = 68 kJ
What effect will a temperature increase of 50°C have on this system at equilibrium?
A) The partial pressure of hydrogen bromide will increase.
B) The partial pressure of hydrogen will increase.
C) The partial pressure of hydrogen bromide and bromine will increase.
D) There will be no effect on the partial pressure of any of the gases.
E) Need to know the initial pressure, volume, and temperature before any of the above predictions can be made.
H2(g) + Br2(g) ΔH°rxn = 68 kJWhat effect will a temperature increase of 50°C have on this system at equilibrium?
A) The partial pressure of hydrogen bromide will increase.
B) The partial pressure of hydrogen will increase.
C) The partial pressure of hydrogen bromide and bromine will increase.
D) There will be no effect on the partial pressure of any of the gases.
E) Need to know the initial pressure, volume, and temperature before any of the above predictions can be made.
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72
At 450°C, tert-butyl alcohol decomposes into water and isobutene. (CH3)3COH(g) (CH3)2CCH2(g) + H2O(g)
A reaction vessel contains these compounds at equilibrium. What will happen if the volume of the container is reduced by 50% at constant temperature?
A) The forward reaction will proceed to reestablish equilibrium.
B) The reverse reaction will proceed to reestablish equilibrium.
C) No change occurs.
D) The equilibrium constant will increase.
E) The equilibrium constant will decrease.
(CH3)2CCH2(g) + H2O(g)A reaction vessel contains these compounds at equilibrium. What will happen if the volume of the container is reduced by 50% at constant temperature?
A) The forward reaction will proceed to reestablish equilibrium.
B) The reverse reaction will proceed to reestablish equilibrium.
C) No change occurs.
D) The equilibrium constant will increase.
E) The equilibrium constant will decrease.
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73
Stearic acid, nature's most common fatty acid, dimerizes when dissolved in hexane: 2C17H35COOH (C17H35COOH)2 ΔH°rxn = -172 kJ
The equilibrium constant for this reaction at 28°C is 2900. Estimate the equilibrium constant at 38°C.
A) 4.7 × 105
B) 2.6 × 104
C) 1.9 × 103
D) 3.2 × 102
E) 18
(C17H35COOH)2 ΔH°rxn = -172 kJThe equilibrium constant for this reaction at 28°C is 2900. Estimate the equilibrium constant at 38°C.
A) 4.7 × 105
B) 2.6 × 104
C) 1.9 × 103
D) 3.2 × 102
E) 18
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74
The reaction of nitric oxide to form dinitrogen oxide and nitrogen dioxide is exothermic. 3NO(g) N2O(g) + NO2(g) + heat
What effect will be seen if the temperature of the system at equilibrium is raised by 25°C?
A) The partial pressure of NO will increase.
B) The partial pressure of NO will decrease.
C) The partial pressure of NO2 will increase.
D) The partial pressures of NO and N2O will increase.
E) All three partial pressures will increase.
N2O(g) + NO2(g) + heatWhat effect will be seen if the temperature of the system at equilibrium is raised by 25°C?
A) The partial pressure of NO will increase.
B) The partial pressure of NO will decrease.
C) The partial pressure of NO2 will increase.
D) The partial pressures of NO and N2O will increase.
E) All three partial pressures will increase.
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75
The following reaction is at equilibrium at a pressure of 1 atm, in a closed container. NaOH(s) + CO2(g) NaHCO3(s) ΔH°rxn < 0
Which, if any, of the following actions will decrease the concentration of CO2 gas present at equilibrium?
A) adding N2 gas to double the pressure
B) adding more solid NaOH
C) increasing the volume of the container
D) lowering the temperature
E) None of these choices are correct.
NaHCO3(s) ΔH°rxn < 0Which, if any, of the following actions will decrease the concentration of CO2 gas present at equilibrium?
A) adding N2 gas to double the pressure
B) adding more solid NaOH
C) increasing the volume of the container
D) lowering the temperature
E) None of these choices are correct.
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76
Ethane can be formed by reacting acetylene with hydrogen. C2H2(g) + 2H2(g) C2H6(g) ΔH°rxn = -311 kJ
Under which reaction conditions would you expect to have the greatest equilibrium yield of ethane?
A) high temperature, high pressure
B) low temperature, high pressure
C) high temperature, low pressure
D) low temperature, low pressure
E) None of these choices are correct.
C2H6(g) ΔH°rxn = -311 kJUnder which reaction conditions would you expect to have the greatest equilibrium yield of ethane?
A) high temperature, high pressure
B) low temperature, high pressure
C) high temperature, low pressure
D) low temperature, low pressure
E) None of these choices are correct.
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77
A container was charged with hydrogen, nitrogen, and ammonia gases at 120°C and the system was allowed to reach equilibrium. What will happen if the volume of the container is increased at constant temperature? 3H2(g) + N2(g) 2NH3(g)
A) There will be no effect.
B) More ammonia will be produced at the expense of hydrogen and nitrogen.
C) Hydrogen and nitrogen will be produced at the expense of ammonia.
D) The equilibrium constant will increase.
E) The equilibrium constant will decrease.
2NH3(g)A) There will be no effect.
B) More ammonia will be produced at the expense of hydrogen and nitrogen.
C) Hydrogen and nitrogen will be produced at the expense of ammonia.
D) The equilibrium constant will increase.
E) The equilibrium constant will decrease.
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78
The reaction system CS2(g) + 4H2(g) CH4(g) + 2H2S(g)
Is at equilibrium. Which of the following statements describes the behavior of the system if the partial pressure of carbon disulfide is reduced?
A) As equilibrium is reestablished, the partial pressure of carbon disulfide increases.
B) As equilibrium is reestablished, the partial pressure of hydrogen decreases.
C) As equilibrium is reestablished, the partial pressure of methane, CH4, increases.
D) As equilibrium is reestablished, the partial pressures of hydrogen and hydrogen sulfide decrease.
E) As equilibrium is reestablished, all the partial pressures will increase.
CH4(g) + 2H2S(g)Is at equilibrium. Which of the following statements describes the behavior of the system if the partial pressure of carbon disulfide is reduced?
A) As equilibrium is reestablished, the partial pressure of carbon disulfide increases.
B) As equilibrium is reestablished, the partial pressure of hydrogen decreases.
C) As equilibrium is reestablished, the partial pressure of methane, CH4, increases.
D) As equilibrium is reestablished, the partial pressures of hydrogen and hydrogen sulfide decrease.
E) As equilibrium is reestablished, all the partial pressures will increase.
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79
The following reaction is at equilibrium in a sealed container. N2(g) + 3H2(g) 2NH3(g) ΔH°rxn < 0
Which, if any, of the following actions will increase the value of the equilibrium constant, Kc?
A) adding a catalyst
B) adding more N2
C) increasing the pressure
D) lowering the temperature
E) None of these choices are correct.
2NH3(g) ΔH°rxn < 0Which, if any, of the following actions will increase the value of the equilibrium constant, Kc?
A) adding a catalyst
B) adding more N2
C) increasing the pressure
D) lowering the temperature
E) None of these choices are correct.
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80
Magnesium carbonate dissociates to magnesium oxide and carbon dioxide at elevated temperatures. MgCO3(s) MgO(s) + CO2(g)
A reaction vessel contains these compounds in equilibrium at 300°C. What will happen if the volume of the container is reduced by 25% at 300°C?
A) The partial pressure of carbon dioxide present at equilibrium will increase.
B) The partial pressure of carbon dioxide present at equilibrium will decrease.
C) The partial pressure of carbon dioxide at equilibrium will be unchanged.
D) The equilibrium constant will have to decrease to compensate for the decrease in volume.
E) More information is needed in order to make a valid judgment.
MgO(s) + CO2(g)A reaction vessel contains these compounds in equilibrium at 300°C. What will happen if the volume of the container is reduced by 25% at 300°C?
A) The partial pressure of carbon dioxide present at equilibrium will increase.
B) The partial pressure of carbon dioxide present at equilibrium will decrease.
C) The partial pressure of carbon dioxide at equilibrium will be unchanged.
D) The equilibrium constant will have to decrease to compensate for the decrease in volume.
E) More information is needed in order to make a valid judgment.
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