Deck 15: Chemical Equilibrium

Question 1

The equilibrium expression for K_p for the reaction below is ________. 2O₃ (g) 3O₂ (g)

A)
B)
C)
D)
E)

Answer 1

Question 2

The K_eq for the equilibrium below is 7.52 × 10^-2 at 480.0 °C. 2Cl₂ (g)+ 2H₂O (g) 4HCl (g)+ O₂ (g)
What is the value of K_eq at this temperature for the following reaction?
2HCl (g)+ O₂ (g) Cl₂ (g)+ H₂O (g)

A)13.3
B)3.65
C)-0.0376
D)5.66 × 10^-3
E)0.274

Answer 2

3.65

Question 3

Which of the following expressions is the correct equilibrium-constant expression for the reaction below?
(NH₄)₂Se (s) 2NH₃ (g)+ H₂Se (g)

A)[NH₃][H₂Se] / [(NH₄)₂Se]
B)[(NH₄)₂Se] / [NH₃]²[H₂Se]
C)1 / [(NH₄)₂Se]
D)[NH₃]²[H₂Se]
E)[NH₃]²[H₂Se] / [(NH₄)₂Se]

Answer 3

[NH₃]²[H₂Se]

Question 4

The K_eq for the equilibrium below is 50. H₂ (g)+ I₂ (g) 2HI (g)
What is the value of K_eq for the following reaction?
2HI (g) H₂ (g)+ I₂ (g)

A)100
B)0.50
C)0.020
D)2500
E)-50

Question 5

What role did Karl Bosch play in development of the Haber-Bosch process?

A)He discovered the reaction conditions necessary for formation of ammonia.
B)He originally isolated ammonia from camel dung and found a method for purifying it.
C)Haber was working in his lab with his instructor at the time he worked out the process.
D)He developed the equipment necessary for industrial production of ammonia.
E)He was the German industrialist who financed the research done by Haber.

Question 6

The equilibrium constant for reaction 1 is K.The equilibrium constant for reaction 2 is ________. (1)SO₂ (g)+ (1/2)O₂ (g) SO₃ (g)
(2)2SO₃ (g) 2SO₂ (g)+ O₂ (g)

A)K²
B)2K
C)1/2K
D)1/K²
E)-K²

Question 7

The K_eq for the equilibrium below is 5.4 × 10¹³ at 480.0 °C. 2NO (g)+ O₂ (g) 2NO₂ (g)
What is the value of K_eq at this temperature for the following reaction?
2NO₂ (g) 2NO (g)+ O₂ (g)

A)5.4 × 10^-13
B)1.9 × 10^-14
C)5.4 × 10¹³
D)5.66 × 10^-3
E)none of the above

Question 8

Fritz Haber was awarded the ________ Nobel Prize in chemistry for his development of a process for synthesizing ammonia directly from nitrogen and hydrogen.

A)1954
B)1918
C)1933
D)1900
E)1912

Question 9

Which of the following expressions is the correct equilibrium-constant expression for the following reaction?
CO₂ (g)+ 2H₂ (g) CH₃OH (g)

A)
B)
C)
D)
E)

Question 10

The K_eq for the equilibrium below is 50. H₂ (g)+ I₂ (g) 2HI (g)
What is the value of K_eq for the following reaction? H₂ (g)+ I₂ (g) HI (g)

A)25
B)2500
C)7.07
D)100
E)-50

Question 11

The equilibrium-constant expression depends on the ________ of the reaction.

A)stoichiometry
B)mechanism
C)stoichiometry and mechanism
D)the quantities of reactants and products initially present
E)temperature

Question 12

Given the following reaction at equilibrium,if K_c = 1.90 × 10¹⁹ at 25.0 °C,K_p = ________. H₂ (g)+ Br₂ (g) 2 HBr (g)

A)5.26 × 10^-20
B)1.56 × 10⁴
C)6.44 × 10⁵
D)1.90 × 10¹⁹
E)none of the above

Question 13

Which of the following expressions is the correct equilibrium-constant expression for the equilibrium between dinitrogen tetroxide and nitrogen dioxide?
N₂O₄ (g) 2NO₂ (g)

A)
B)
C)
D)[NO₂][N₂O₄]
E)[NO₂]²[N₂O₄]

Question 14

Which one of the following will change the value of an equilibrium constant?

A)changing temperature
B)adding other substances that do not react with any of the species involved in the equilibrium
C)varying the initial concentrations of reactants
D)varying the initial concentrations of products
E)changing the volume of the reaction vessel

Question 15

At equilibrium,________.

A)all chemical reactions have ceased
B)the rates of the forward and reverse reactions are equal
C)the rate constants of the forward and reverse reactions are equal
D)the value of the equilibrium constant is 1
E)the limiting reagent has been consumed

Question 16

Which of the following expressions is the correct equilibrium-constant expression for the reaction below?
CO₂ (s)+ H₂O (l) H⁺ (aq)+ HCO₃^- (aq)

A)[H⁺][HCO₃^-] / [CO₂]
B)[CO₂] / [H⁺][HCO₃^-]
C)[H⁺][HCO₃^-] / [CO₂][H₂O]
D)[CO₂][H₂O] / [H⁺][HCO₃^-]
E)[H⁺][HCO₃^-]

Question 17

The equilibrium expression for K_p for the reaction below is ________. N₂ (g)+ O₂ (g) 2NO (g)

A)
B)
C)
D)
E)none of the above

Question 18

Which of the following expressions is the correct equilibrium-constant expression for the reaction below?
2SO₂ (g)+ O₂ (g) 2SO₃ (g)

A)[SO₃] / [SO₂][O₂]
B)[SO₂] / [SO₃]
C)[SO₃]² / [SO₂]²[O₂]
D)[SO₃]² / [SO₂]²[O₂]²
E)[SO₃] / [SO₂][O₂]²

Question 19

Which one of the following is true concerning the Haber process?

A)It is a process used for shifting equilibrium positions to the right for more economical chemical synthesis of a variety of substances.
B)It is a process used for the synthesis of ammonia.
C)It is another way of stating Le Châtelier's principle.
D)It is an industrial synthesis of sodium chloride that was discovered by Karl Haber.
E)It is a process for the synthesis of elemental chlorine.

Question 20

Which of the following expressions is the correct equilibrium-constant expression for the reaction below?
HF (aq)+ H₂O (l) H₃O⁺ (aq)+ F^- (aq)

A)[HF][H₂O] / [H₃O⁺][F^-]
B)1 / [HF]
C)[H₃O⁺][F^-] / [HF][H₂O]
D)[H₃O⁺][F^-] / [HF]
E)[F^-] / [HF]

Question 21

Based on Le Châtelier's principle,increasing pressure at constant temperature in the following reaction will not change the concentrations of reactants and products.

A)N₂O₄ (g) 2NO₂ (g)
B)N₂ (g)+ O₂ (g) 2NO (g)
C)N₂ (g)+ 2O₂ (g) 2NO₂ (g)
D)N₂ (g)+ 3H₂ (g) 2NH₃ (g)
E)2N₂ (g)+ O₂ (g) 2N₂O (g)

Question 22

Consider the following reaction at equilibrium. 2CO₂ (g) 2CO (g)+ O₂ (g)ΔH° = -514 kJ
Le Châtelier's principle predicts that the equilibrium partial pressure of CO (g)can be maximized by carrying out the reaction ________.

A)at high temperature and high pressure
B)at high temperature and low pressure
C)at low temperature and low pressure
D)at low temperature and high pressure
E)in the presence of solid carbon

Question 23

The effect of a catalyst on an equilibrium is to ________.

A)increase the rate of the forward reaction only
B)increase the equilibrium constant so that products are favored
C)slow the reverse reaction only
D)increase the rate at which equilibrium is achieved without changing the composition of the equilibrium mixture
E)shift the equilibrium to the right

Question 24

The equilibrium constant for the gas phase reaction H₂ (g)+ I₂ (g) 2HI (g)
Is K_eq = 50 at 25 °C.At equilibrium,________.

A)products predominate
B)reactants predominate
C)roughly equal amounts of products and reactants are present
D)only products are present
E)only reactants are present

Question 25

In which of the following reactions would increasing pressure at constant temperature change the concentrations of reactants and products,based on Le Châteliers principle?

A)N₂ (g)+ 3H₂ (g) 2NH₃ (g)
B)N₂O₄ (g) 2NO₂ (g)
C)N₂ (g)+ 2O₂ (g) 2NO₂ (g)
D)2N₂ (g)+ O₂ (g) 2 O (g)
E)all of the above

Question 26

Consider the following reaction at equilibrium: 2NH₃ (g) N₂ (g)+ 3H₂ (g)
Le Châtelier's principle predicts that the moles of in the reaction container will increase with ________.

A)some removal of from the reaction vessel (V and T constant)
B)a decrease in the total pressure (T constant)
C)addition of some to the reaction vessel (V and T constant)
D)a decrease in the total volume of the reaction vessel (T constant)
E)an increase in total pressure by the addition of helium gas (V and T constant)

Question 27

Which reaction will shift to the left in response to a decrease in volume?

A)2HI (g) H₂ (g)+ I₂ (g)
B)H₂ (g)+ Cl₂ (g) 2 HCl (g)
C)N₂ (g)+ 3H₂ (g) 2 NH₃ (g)
D)2 SO₃ (g) 2 SO₂ (g)+ O₂ (g)
E)4 Fe (s)+ 3 O₂ (g) 2 Fe₂O₃ (s)

Question 28

The equilibrium constant for the gas phase reaction 2SO₂ (g)+ O₂ (g) 2SO₃ (g)
Is K_eq = 2.80 × 10² at 999 K.At equilibrium,________.

A)products predominate
B)reactants predominate
C)roughly equal amounts of products and reactants are present
D)only products are present
E)only reactants are present

Question 29

How is the reaction quotient used to determine whether a system is at equilibrium?

A)The reaction quotient must be satisfied for equilibrium to be achieved.
B)At equilibrium, the reaction quotient is undefined.
C)The reaction is at equilibrium when Q < K_eq.
D)The reaction is at equilibrium when Q > K_eq.
E)The reaction is at equilibrium when Q = K_eq.

Question 30

The equilibrium constant for the gas phase reaction 2SO₃ (g) 2SO₂ (g)+ O₂ (g)
Is K_eq = 3.6 × 10^-3 at 999 K.At equilibrium,________.

A)products predominate
B)reactants predominate
C)roughly equal amounts of products and reactants are present
D)only products are present
E)only reactants are present

Question 31

The equilibrium constant for the gas phase reaction N₂ (g)+ 3H₂ (g) 2NH₃ (g)
Is K_eq = 4.34 × 10^-3 at 300 °C.At equilibrium,________.

A)products predominate
B)reactants predominate
C)roughly equal amounts of products and reactants are present
D)only products are present
E)only reactants are present

Question 32

Which reaction will shift to the right in response to a decrease in volume?

A)N₂ (g)+ 3H₂ (g) 2NH₃ (g)
B)H₂ (g)+ Cl₂ (g) 2 HCl (g)
C)2 SO₃ (g) 2 SO₂ (g)+ O₂ (g)
D)2HI (g) H₂ (g)+ I₂ (g)
E)2 Fe₂O₃ (s) 4 Fe (s)+ 3O₂ (g)

Question 33

Consider the following reaction at equilibrium: 2CO₂ (g) 2CO (g)+ O₂ (g)ΔH° = -514 kJ
Le Châtelier's principle predicts that a decrease in temperature will ________.

A)decrease the partial pressure of O₂ (g)
B)increase the partial pressure of CO₂ (g)
C)decrease the value of the equilibrium constant
D)increase the value of the equilibrium constant
E)decrease the partial pressure of CO

Question 34

At 400 K,the equilibrium constant for the reaction Br₂ (g)+ Cl₂ (g) 2BrCl (g)
Is K_p = 7.0.A closed vessel at 400 K is charged with 1.00 atm of Br₂ (g),1.00 atm of Cl₂ (g),and 2.00 atm of BrCl (g).Use Q to determine which of the statements below is true.

A)The equilibrium partial pressures of Br₂, Cl₂, and BrCl will be the same as the initial values.
B)The equilibrium partial pressure of BrCl (g)will be 4.00 atm.
C)The equilibrium partial pressure of Br₂ will be greater than 1.00 atm.
D)At equilibrium, the total pressure in the vessel will be less than the initial total pressure.
E)The reaction will go to completion since there are equal amounts of Br₂ and Cl₂.

Question 35

The value of K_eq for the equilibrium H₂ (g)+ I₂ (g) 2HI (g)
Is 794 at 25 °C.At this temperature,what is the value of K_eq for the equilibrium below?
HI (g) 1/2 H₂ (g)+ 1/2 I₂ (g)

A)1588
B)28
C)397
D)0.035
E)0.0013

Question 36

The equilibrium-constant expression for the reaction Ti (s)+ 2Cl₂ (g) TiCl₄ (l)
Is given by

A)
B)
C)
D)[Cl₂ (g)]^-2
E)

Question 37

The expression for for the reaction below is ________. 4CuO (s)+ CH₄ (g) CO₂ (g)+ 4Cu (s)+ 2H₂O (g)

A)
B)
C)
D)
E)

Question 38

Which of the following statements is true?

A)Q does not change with temperature.
B)K_eq does not change with temperature, whereas Q is temperature dependent.
C)K does not depend on the concentrations or partial pressures of reaction components.
D)Q does not depend on the concentrations or partial pressures of reaction components.
E)Q is the same as K_eq when a reaction is at equilibrium.

Question 39

The equilibrium constant for the gas phase reaction 2NH₃ (g) N₂ (g)+ 3H₂ (g)
Is K_eq = 230 at 300 °C.At equilibrium,________.

A)products predominate
B)reactants predominate
C)roughly equal amounts of products and reactants are present
D)only products are present
E)only reactants are present

Question 40

The value of K_eq for the equilibrium H₂ (g)+ I₂ (g) 2HI (g)
Is 794 at 25 °C.What is the value of K_eq for the equilibrium below?
1/2 H₂ (g)+ 1/2 I₂ (g) HI (g)

A)397
B)0.035
C)28
D)1588
E)0.0013

Question 41

At 200 °C,the equilibrium constant (K_p)for the conversion of NO to oxygen and nitrogen gas is 2.40 × 10³.A closed vessel is charged with 36.1 atm of NO.At equilibrium,the partial pressure of O₂ is ________ atm.

A)294
B)6.00
C)35.7
D)1.50 × 10^-2
E)17.9

Question 42

Dinitrogentetraoxide partially decomposes into nitrogen dioxide.A 1.00-L flask is charged with of N₂O₄.At equilibrium at 373 K,0.0055 mol of N₂O₄ remains.K_eq for this reaction is ________.

A)2.2 × 10^-4
B)13
C)0.22
D)0.87
E)0.022

Question 43

The value of for the following reaction is 0.25: S (g)+ N (g) S (g)+ NO (g)
The value of at the same temperature for the reaction below is ________.
3S (g)+ 3N (g) 3S (g)+ 3NO (g)

A)1.6 × 10^-2
B)7.5 × 10^-1
C)8.3 × 10^-2
D)6.4 × 10¹
E)0.25

Question 44

The equilibrium constant (K_p)for the interconversion of PCl₅ and PCl₃ is 0.0121.A vessel is charged with PCl₅ giving an initial pressure of 0.123 atm and yields PCl₃ and Cl₂.At equilibrium,the partial pressure of PCl₃ is ________ atm.

A)0.0782
B)0.0330
C)0.0908
D)0.0455
E)0.123

Question 45

In an experiment,0.42 mol of CO and 0.42 mol of H₂ were placed in a 1.00-L reaction vessel to yield CH₃OH.At equilibrium,there were 0.29 mol of CO remaining.K_eq at the temperature of the experiment is ________.

A)2.80
B)17.5
C)0.357
D)14.5
E)none of the above

Question 46

The K_eq for the equilibrium below is 0.112 at 700.0 °C. SO₂ (g)+ O₂ (g) SO₃ (g)
What is the value of K_eq at this temperature for the following reaction?
2SO₂ (g)+ O₂ (g) 2SO₃ (g)

A)1.25 × 10^-2
B)2.24 × 10^-1
C)7.97 × 10¹
D)4.46
E)0.112

Question 47

Given the following reaction at equilibrium at 300.0 K: NH₄HS (s) NH₃ (g)+ H₂S (g)
If pNH₃ = pH₂S = 0.105 atm,K_p = ________.

A).0110
B)4.99 × 10^-4
C).105
D).0821
E)5.66 × 10^-3

Question 48

A reaction vessel is charged with hydrogen iodide,which partially decomposes to molecular hydrogen and iodine: 2HI (g) H₂(g)+ I₂(g)
When the system comes to equilibrium at 425 °C,P_HI = 0.708 atm,and = The value of K_p at this temperature is ________.

A)6.80 × 10^-2
B)1.30 × 10^-2
C)54.3
D)1.84 × 10^-2
E)K_p cannot be calculated for this gas reaction when the volume of the reaction vessel is not given.

Question 49

Given the following reaction at equilibrium,if K_p = 1.10 at 250.0 °C,K_c = ________. PCl₅ (g) PCl₃ (g)+ Cl₂ (g)

A)3.90 × 10^-6
B)2.56 × 10^-2
C)1.10
D)42.9
E)47.2

Question 50

Given the following reaction at equilibrium,if K_c = 5.84 x 10⁵ at 230.0 °C,K_p = ________. 2NO (g)+ O₂ (g) (g)

A)3.67 × 10^-2
B)1.41 × 10⁴
C)6.44 × 10⁵
D)2.40 × 10⁶
E)2.41 × 10⁷

Question 51

Which of the following expressions is the correct equilibrium-constant expression for the equilibrium between dinitrogen tetroxide and nitrogen dioxide?
5N₂O4(g) 10NO₂ (g)

A)[NO₂]¹⁰/[N₂O₄]⁵
B)[N₂O₄]¹⁰/[NO₂]⁵
C)[NO₂]⁵/[N₂O₄]¹⁰
D)[NO₂]⁵/[N₂O₄]⁵
E)[N₂O₄]⁵/[NO₂]⁵

Question 52

The value of K_eq for the equilibrium CO₂ (g)+ 2H₂ (g) CH₃OH (g)
Is 14.5 at 483 °C.What is the value of K_eq for the equilibrium below?
1/2 CO₂ + H₂ (g) 1/2 CH₃OH (g)

A)7.30
B)7.35
C)0.136
D)3.81
E)6.90 × 10^-2

Question 53

The K_eq for the equilibrium below is 5.4 × 10¹³ at 480.0 °C. 2NO (g)+ O₂ (g) 2NO₂ (g)
What is the value of K_eq at this temperature for the following reaction?
4NO (g)+ 2O₂ (g) 4NO₂ (g)

A)2.9 × 10²⁷
B)8.5 × 10⁵⁴
C)3.4 × 10^-28
D)-1.1 × 10¹⁴
E)5.4 × 10¹³

Question 54

The K_eq for the equilibrium below is 7.52 × 10^-2 at 480.0 °C. 2Cl₂ (g)+ 2H₂O (g) 4HCl (g)+ O₂ (g)
What is the value of K_eq at this temperature for the following reaction?
8HCl (g)+ 2O₂ (g) 4Cl₂ (g)+ 4H₂O (g)

A)1.77 × 10²
B)5.66 × 10^-3
C)1.50 × 10^-1
D)-7.52 × 10^-2
E)7.52 × 10^-2

Question 55

Consider the following chemical reaction: CO (g)+ 2H₂(g) CH₃OH(g)
At equilibrium in a particular experiment,the concentrations of CO and H₂ were and respectively.What is the equilibrium concentration of CH₃OH?
The value of K_eq for this reaction is 14.5 at the temperature of the experiment.

A)14.5
B)7.61 × 10^-3
C)2.82 × 10^-1
D)3.72 × 10^-3
E)1.34 × 10^-3

Question 56

The value of K_eq for the equilibrium H₂ (g)+ I₂ (g) 2HI (g)
Is 54.0 at 427 °C.What is the value of K_eq for the equilibrium below?
HI (g) 1/2 H₂ (g)+ 1/2 I₂(g)

A)27
B)7.35
C)0.136
D)2.92 × 10³
E)3.43 × 10^-4

Question 57

A sealed 1.0 L flask is charged with 0.500 mol of I₂ and 0.500 mol of Br₂.An equilibrium reaction ensues: I₂ (g)+ Br₂ (g) 2IBr (g)
When the container contents achieve equilibrium,the flask contains 0.84 mol of IBr.The value of is ________.

A)11
B)4.0
C)110
D)6.1
E)2.8

Question 58

Acetic acid is a weak acid that dissociates into the acetate ion and a proton in aqueous solution: HC₂H₃O₂ (aq) C₂H₃O₂^- (aq)+ H⁺ (aq)
At equilibrium at 25 °C a 0.100 M solution of acetic acid has the following concentrations: and The equilibrium constant,K_eq,for the ionization of acetic acid at is ________.

A)5.71 × 10⁴
B)0.100
C)1.75 × 10^-7
D)1.79 × 10^-5
E)5.71 × 10⁶

Question 59

Given the following reaction at equilibrium at 450.0 °C: CaCO₃ (s) CaO (s)+ CO₂ (g)
If pCO₂ = 0.0155 atm,K_c = ________.

A)155
B)0.0821
C)0.920
D)2.61 × 10^-4
E)9.20

Question 60

The value of K_eq for the equilibrium N₂ (g)+ O₂ (g) 2 NO (g)
Is 4.2 × 10^-31 at 27 °C.What is the value of K_eq for the equilibrium below?
4 NO (g) 2 N₂ (g)+ 2 O₂ (g)

A)5.7 × 10⁶⁰
B)8.4 × 10^-31
C)4.2 × 10³¹
D)8.4 × 10³¹
E)none of the above

Question 61

Consider the following reaction at equilibrium: 2C (g) 2CO (g)+ (g)ΔH° = -514 kJ
Le Châtelier's principle predicts that removing (g)to the reaction container will ________.

A)increase the partial pressure of CO
B)decrease the partial pressure of CO
C)increase the partial pressure of CO₂
D)increase the value of the equilibrium constant
E)decrease the value of the equilibrium constant

Question 62

The reaction below is exothermic: 2SO₂ (g)+ O₂ (g) 2SO₃ (g)
Le Châtelier's Principle predicts that ________ will result in an increase in the number of moles of in the reaction container.

A)increasing the amount of SO₂
B)decreasing the pressure
C)increasing the temperature
D)removing some oxygen
E)increasing the volume of the container

Question 63

At elevated temperatures,molecular hydrogen and molecular bromine react to partially form hydrogen bromide: H₂ (g)+ Br₂ (g) 2HBr (g)
A mixture of 0.682 mol of H₂ and 0.440 mol of Br₂ is combined in a reaction vessel with a volume of At equilibrium at 700 K,there are 0.546 mol of H₂ present.At equilibrium,there are ________ mol of Br₂ present in the reaction vessel.

A)0.000
B)0.440
C)0.546
D)0.136
E)0.304

Question 64

The K_eq for the equilibrium below is 7.16 × 10^-2 at 440.0 °C. 2Cl₂ (g)+ 2H₂O (g) 4HCl (g)+ O₂ (g)
What is the value of K_eq at this temperature for the following reaction?
Cl₂ (g)+ H₂O (g) 2HCl (g)+ O₂ (g)

A)0.0716
B)5.13 × 10^-3
C)0.268
D)0.0376
E)0.150

Question 65

= 0.0198 at 721 K for the reaction 2HI (g) (g)+ (g)
In a particular experiment,the partial pressures of and at equilibrium are 0.678 and 0.788 atm,respectively.The partial pressure of HI is ________ atm.

A)7.87
B)27.0
C)5.19
D)0.103
E)0.0106

Question 66

Phosphorous trichloride and phosphorous pentachloride equilibrate in the presence of molecular chlorine according to the reaction: (g)+ (g)→ (g) An equilibrium mixture at 450 K contains = 0.224 atm, = 0.284 atm,and = 4.24 atm.What is the value of K_p at this temperature?

A)66.7
B)1.50 ×
C)2.70 × 10^-1
D)3.74
E)8.36

Question 67

For the endothermic reaction CaCO₃ (s) CaO (s)+ CO₂ (g)
Le Châtelier's principle predicts that ________ will result in an increase in the number of moles of

A)increasing the temperature
B)decreasing the temperature
C)increasing the pressure
D)removing some of the CaCO₃(s)
E)none of the above

Question 68

The value of K_eq for the following reaction is 0.26: A (g)+ B (g) C (g)+ D (g)
The value of K_eq at the same temperature for the reaction below is ________.
2A (g)+ 2B (g) 2C (g)+ 2D (g)

A)0.068
B)0.52
C)1.2
D)0.065
E)0.26

Question 69

In the coal-gasification process,carbon monoxide reacts with water to produce carbon dioxide and hydrogen gas.In an experiment,0.35 mol of CO and 0.40 mol of H₂O were placed in a 1.00-L reaction vessel.At equilibrium,there were 0.22 mol of CO remaining.K_eq at the temperature of the experiment is ________.

A)5.5
B)0.28
C)0.75
D)3.5
E)1.0

Question 70

Hydrogen and iodine gas react to produce hydrogen iodide gas.What is the value of for this reaction if at equilibrium the concentrations of , ,and HI were and respectively?

A)23
B)34
C)63
D)0.0090
E)5.1

Question 71

At 24°C,K_p = 0.080 for the equilibrium: NH₄HS (s) NH₃ (g)+ H₂S (g)
A sample of solid NH₄HS is placed in a closed vessel and allowed to equilibrate.Calculate the equilibrium partial pressure (atm)of ammonia,assuming that some solid NH₄HS remains.

A)0.28
B)0.080
C)0.052
D)0.0049
E)3.8

Question 72

Dinitrogen tetroxide partially decomposes according to the following equilibrium: (g)→ (g) A 1.000-L flask is charged with 9.20 × 10^-3 mol of .At equilibrium,5.98 × 10^-3 mol of remains. for this reaction is ________.

A)0.183
B)0.197
C)0.212
D)6.94 ×
E)2.96 × 10^-5

Question 73

The value of K_eq for the following reaction is 0.16: A (g)+ B (g) C (g)+ D (g)
The value of K_eq at the same temperature for the reaction below is ________.
3C (g)+ 3D (g) 3A (g)+ 3B (g)

A)2.4 × 10²
B)2.1
C)4.1 × 10^-3
D)5.3 × 10^-2
E)6.3

Question 74

At 1000.0 K,the equilibrium constant for the reaction 2NO (g)+ Br₂ (g) 2NOBr (g)
Is K_p = 0.016.Calculate K_p for the reverse reaction,
2NOBr (g) 2NO (g)+ Br₂ (g).

A)0.016
B)1.6 × 10^-4
C)63
D)0.99
E)1.1

Question 75

Consider the following reaction at equilibrium: 2N (g) (g)+ 3 (g)ΔH° = +92.4 kJ
Le Châtelier's principle predicts that removing to the system at equilibrium will result in ________.

A)an increase in the concentration of H₂
B)a decrease in the concentration of H₂
C)removal of all of the H₂
D)a lower partial pressure of H₂
E)an increase in the value of the equilibrium constant

Question 76

Nitrosyl bromide decomposes according to the following equation. 2NOBr (g) 2NO (g)+ (g)
A sample of NOBr (0.64 mol)was placed in a 1.00-L flask containing no NO or .At equilibrium the flask contained of NOBr.How many moles of NO and ,respectively,are in the flask at equilibrium?

A)0.48, 0.24
B)0.48, 0.48
C)0.16, 0.08
D)0.16, 0.16
E)0.24, 0.42

Question 77

The value of K_eq for the following reaction is 0.50: A (g)+ 2B (g) C (g)+ 4D (g)
The value of K_eq at the same temperature for the reaction below is ________.
1/2A (g)+ B (g) 1/2C (g)+ 2D (g)

A)7.1 × 10^-1
B)2.5 × 10^-1
C)0.25
D)1.0
E)0.50

Question 78

The expression of K_eq for the following reaction will not include ________. A(g)+ B(g) C(l)+ D(g)

A)[C]
B)[A]
C)[B]
D)[D]
E)none of the above

Question 79

Carbon monoxide and chlorine gas react to produce COCl₂ gas.The for the reaction is 1.49 × 10⁸ at 100.0 °C: In an equilibrium mixture of the three gases, = = 7.70 × 10^-4 atm.The partial pressure of the product,phosgene ( ),is ________ atm.

A)2.51 × 10¹⁴
B)3.98 × 10^-15
C)1.15 × 10⁵
D)8.83 × 10¹
E)1.92 × 10¹¹

Question 80

At 900.0 K,the equilibrium constant (K_p)for the following reaction is 0.345. + (g)→ (g) At equilibrium,the partial pressure of is 36.9 atm and that of is 16.8 atm.The partial pressure of is ________ atm.

A)88.8
B)3.89 ×
C)214
D)5.57 × 10^-4
E)42.4