تكلم مع الذكاء الاصطناعي
Deck 13: Equilibrium
ملء الشاشة (f)
سؤال
Which is the correct equilibrium constant expression for the following reaction? 2C6H6(g) + 15O2(g) 
12CO₂(g) + 6H₂O(g)
A)
B)
C)
D)
E)
12CO₂(g) + 6H₂O(g)A)
B)
C)
D)
E)
سؤال
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 in order to reestablish equilibrium.
B)The reverse reaction will proceed in order 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 in order to reestablish equilibrium.
B)The reverse reaction will proceed in order to reestablish equilibrium.
C)No change occurs.
D)The equilibrium constant will increase.
E)The equilibrium constant will decrease.
سؤال
Write the equilibrium constant expression for the reaction shown. 
A)
B)
C)
D)
E)
A)
B)
C)
D)
E)
سؤال
The reaction system POBr3(g) 
POBr(g) + Br2(g) is at equilibrium.Which of the following statements describes the behavior of the system if POBr is added to the container?
A)POBr will be consumed in order to establish a new equilibrium.
B)The partial pressures of POBr3 and POBr will remain steady while the partial pressure of bromine increases.
C)The partial pressure of bromine will increase while the partial pressure of POBr decreases.
D)The partial pressure of bromine remains steady while the partial pressures of POBr3 and POBr increase.
E)The forward reaction will proceed to establish equilibrium.
POBr(g) + Br2(g) is at equilibrium.Which of the following statements describes the behavior of the system if POBr is added to the container?A)POBr will be consumed in order to establish a new equilibrium.
B)The partial pressures of POBr3 and POBr will remain steady while the partial pressure of bromine increases.
C)The partial pressure of bromine will increase while the partial pressure of POBr decreases.
D)The partial pressure of bromine remains steady while the partial pressures of POBr3 and POBr increase.
E)The forward reaction will proceed to establish equilibrium.
سؤال
For the reaction 2X(g) + Y(g) 
2Z(g), K = 1.00 ×103 at 500 K.If at equilibrium the concentration of X is 0.20 M and the concentration of Y is 0.50 M, what is the equilibrium concentration of Z?
A)2.2 M
B)3.2 M
C)3.5 M
D)4.5 M
E)7.1 M
2Z(g), K = 1.00 ×103 at 500 K.If at equilibrium the concentration of X is 0.20 M and the concentration of Y is 0.50 M, what is the equilibrium concentration of Z?A)2.2 M
B)3.2 M
C)3.5 M
D)4.5 M
E)7.1 M
سؤال
سؤال
Write the equilibrium constant expression for the reaction shown. 2NOCl(g) ⇌ 2NO(g) + Cl2(g)
A)
B)
C)
D)
E)
A)
B)
C)
D)
E)
سؤال
سؤال
Hydrogen peroxide may decompose to form water and oxygen gas according to the following reaction. 2H2O2(g) 
2H2O(g) + O2(g)
In a particular experiment, 1.75 moles of H2O2 were placed in a 2.5-L reaction chamber at 307ºC.After equilibrium was reached, 1.20 moles of H2O2 remained.What is K for the reaction?
A)2.0 × 10−4
B)2.3 × 10−2
C)2.4 × 10-3
D)5.5 × 10−3
E)3.9 × 10−4
2H2O(g) + O2(g)In a particular experiment, 1.75 moles of H2O2 were placed in a 2.5-L reaction chamber at 307ºC.After equilibrium was reached, 1.20 moles of H2O2 remained.What is K for the reaction?
A)2.0 × 10−4
B)2.3 × 10−2
C)2.4 × 10-3
D)5.5 × 10−3
E)3.9 × 10−4
سؤال
At 35ºC, the equilibrium constant for the reaction 2NOCl(g) ![<strong>At 35ºC, the equilibrium constant for the reaction 2NOCl(g) 2NO(g) + Cl<sub>2</sub>(g) is K = 1.6 × 10<sup>−5</sup>.An equilibrium mixture was found to have the following concentrations of Cl<sub>2</sub> and NOCl: [Cl<sub>2</sub>] = 1.2 × 10<sup>−2</sup> M; [NOCl] = 2.8 × 10<sup>−1</sup> M.Calculate the concentration of NO(g) at equilibrium.</strong> A)1.0 × 10<sup>−4</sup> M B)1.0 × 10<sup>−2</sup> M C)2.8 × 10<sup>−1</sup> M D)2.4 × 10<sup>−2</sup> M E)1.6 × 10<sup>−3</sup> M <div style=padding-top: 35px>](https://d2lvgg3v3hfg70.cloudfront.net/TB1849/11ea78cf_0f9c_f81b_8379_d59077930e7e_TB1849_11.jpg)
2NO(g) + Cl2(g) is K = 1.6 × 10−5.An equilibrium mixture was found to have the following concentrations of Cl2 and NOCl: [Cl2] = 1.2 × 10−2 M; [NOCl] = 2.8 × 10−1 M.Calculate the concentration of NO(g) at equilibrium.
A)1.0 × 10−4 M
B)1.0 × 10−2 M
C)2.8 × 10−1 M
D)2.4 × 10−2 M
E)1.6 × 10−3 M
2NO(g) + Cl2(g) is K = 1.6 × 10−5.An equilibrium mixture was found to have the following concentrations of Cl2 and NOCl: [Cl2] = 1.2 × 10−2 M; [NOCl] = 2.8 × 10−1 M.Calculate the concentration of NO(g) at equilibrium.A)1.0 × 10−4 M
B)1.0 × 10−2 M
C)2.8 × 10−1 M
D)2.4 × 10−2 M
E)1.6 × 10−3 M
سؤال
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 K for this reaction? CO(g) + Br2(g) 
COBr2(g)
A)5.23
B)2.14
C)1.17
D)0.467
E)0.191
COBr2(g)A)5.23
B)2.14
C)1.17
D)0.467
E)0.191
سؤال
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 for this reaction?</strong> A)0.309 B)0.601 C)1.66 D)2.25 E)3.24 <div style=padding-top: 35px>](https://d2lvgg3v3hfg70.cloudfront.net/TB1849/11ea78cf_0f9c_82e4_8379_f5364b6c375c_TB1849_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 K for this reaction?
A)0.309
B)0.601
C)1.66
D)2.25
E)3.24
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 for this reaction?A)0.309
B)0.601
C)1.66
D)2.25
E)3.24
سؤال
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.
سؤال
For the nitrogen fixation reaction, 3H2(g) + N2(g) 
2NH3(g), K = 6.0 × 10−2 at 500°C.If 0.250 M H2 and 0.050 M NH3 are present at equilibrium, what is the equilibrium concentration of N2?
A)3.3 M
B)2.7 M
C)0.20 M
D)0.083 M
E)0.058 M
2NH3(g), K = 6.0 × 10−2 at 500°C.If 0.250 M H2 and 0.050 M NH3 are present at equilibrium, what is the equilibrium concentration of N2?A)3.3 M
B)2.7 M
C)0.20 M
D)0.083 M
E)0.058 M
سؤال
At elevated temperatures, hydrogen iodide may decompose to form hydrogen gas and iodine gas, as follows. 2HI(g) ![<strong>At elevated temperatures, hydrogen iodide may decompose to form hydrogen gas and iodine gas, as follows. 2HI(g) H<sub>2</sub>(g) + I<sub>2</sub>(g) In a particular experiment, the concentrations at equilibrium were measured to be [HI] = 0.85 mol/L, [I<sub>2</sub>] = 0.60 mol/L, and [H<sub>2</sub>] = 0.27 mol/L.What is K for the above reaction?</strong> A)5.3 B)0.22 C)4.5 D)0.19 E)1.6× 10<sup>2</sup> <div style=padding-top: 35px>](https://d2lvgg3v3hfg70.cloudfront.net/TB1849/11ea78cf_0f9c_82e3_8379_812b10ac22ec_TB1849_11.jpg)
H2(g) + I2(g)
In a particular experiment, the concentrations at equilibrium were measured to be [HI] = 0.85 mol/L, [I2] = 0.60 mol/L, and [H2] = 0.27 mol/L.What is K for the above reaction?
A)5.3
B)0.22
C)4.5
D)0.19
E)1.6× 102
H2(g) + I2(g)In a particular experiment, the concentrations at equilibrium were measured to be [HI] = 0.85 mol/L, [I2] = 0.60 mol/L, and [H2] = 0.27 mol/L.What is K for the above reaction?
A)5.3
B)0.22
C)4.5
D)0.19
E)1.6× 102
سؤال
سؤال
سؤال
A 6.0-L vessel was found to contain 1.0 mol BrCl3, 2.0 mol Br2 and 6.0 mol Cl2.What is the equilibrium constant, K, for this equilibrium mixture for the reaction 2BrCl3(g) 
Br2(g) + 3Cl2(g)?
A)0.014
B)108
C)18
D)12
E)432
Br2(g) + 3Cl2(g)?A)0.014
B)108
C)18
D)12
E)432
سؤال
سؤال
Which is the correct equilibrium constant expression for the following reaction? 2BrCl3(g) ![<strong>Which is the correct equilibrium constant expression for the following reaction? 2BrCl<sub>3</sub>(g) Br<sub>2</sub>(g) + 3Cl<sub>2</sub>(g) </strong> A) K<sub>c</sub> = [Br<sub>2</sub>] [Cl<sub>2</sub>]/[BrCl<sub>3</sub>] B) K<sub>c</sub> = [Br<sub>2</sub>] [Cl<sub>2</sub>]<sup>5</sup>/[BrCl<sub>3</sub>]<sup>2</sup> C) K<sub>c</sub> = [Br<sub>2</sub>] [Cl<sub>2</sub>]<sup>3</sup>/[BrCl<sub>3</sub>]<sup>2</sup> D) K<sub>c</sub> = [BrCl<sub>3</sub>]<sup>2</sup>/([Br<sub>2</sub>] × [Cl<sub>2</sub>]3) E) K<sub>c</sub> = 2[BrCl<sub>3</sub>]<sup><sub>2</sub></sup>/([Br<sup>2</sup>] × 3[Cl2]<sup>3</sup>) <div style=padding-top: 35px>](https://d2lvgg3v3hfg70.cloudfront.net/TB1849/11ea78cf_0f9c_0da6_8379_c52b0a42d726_TB1849_11.jpg)
Br2(g) + 3Cl2(g)
A) Kc = [Br2] [Cl2]/[BrCl3]
B) Kc = [Br2] [Cl2]5/[BrCl3]2
C) Kc = [Br2] [Cl2]3/[BrCl3]2
D) Kc = [BrCl3]2/([Br2] × [Cl2]3)
E) Kc = 2[BrCl3]2/([Br2] × 3[Cl2]3)
Br2(g) + 3Cl2(g) A) Kc = [Br2] [Cl2]/[BrCl3]
B) Kc = [Br2] [Cl2]5/[BrCl3]2
C) Kc = [Br2] [Cl2]3/[BrCl3]2
D) Kc = [BrCl3]2/([Br2] × [Cl2]3)
E) Kc = 2[BrCl3]2/([Br2] × 3[Cl2]3)
سؤال
When the following reaction is at equilibrium 2NOCl(g) ![When the following reaction is at equilibrium 2NOCl(g) 2NO(g) + Cl<sub>2</sub>(g) then [NO]<sup>2</sup> [Cl<sub>2</sub>] = K [NOCl]<sup>2</sup>.<div style=padding-top: 35px>](https://d2lvgg3v3hfg70.cloudfront.net/TB1849/11ea78cf_0f9d_1f2c_8379_217481861122_TB1849_11.jpg)
2NO(g) + Cl2(g)
then [NO]2 [Cl2] = K [NOCl]2.
2NO(g) + Cl2(g)then [NO]2 [Cl2] = K [NOCl]2.
سؤال
Which reaction shown will have the highest concentration of products at equilibrium?
A)
B)
C)
D)
E)
A)
B)
C)
D)
E)
سؤال
Determine the balanced chemical equation that corresponds to the given equilibrium expression. 
A)
B)
C)
D)
E)
A)
B)
C)
D)
E)
سؤال
If the system 3H2(g) + N2(g) 
2NH3(g) is at equilibrium and more N2 is added, a net reaction that consumes some of the added N2 will occur until a new equilibrium is reached.
2NH3(g) is at equilibrium and more N2 is added, a net reaction that consumes some of the added N2 will occur until a new equilibrium is reached. سؤال
سؤال
Determine the balanced chemical equation that corresponds to the given equilibrium expression. 
A)
B)
C)
D)
E)
A)
B)
C)
D)
E)
سؤال
The equilibrium constant expression for the reaction CuO(s) + H2(g) ![The equilibrium constant expression for the reaction CuO(s) + H<sub>2</sub>(g) Cu(s) + H<sub>2</sub>O(g) is K = [H<sub>2</sub>]/[H<sub>2</sub>O].<div style=padding-top: 35px>](https://d2lvgg3v3hfg70.cloudfront.net/TB1849/11ea78cf_0f9d_1f2d_8379_31b5eef2f1c9_TB1849_11.jpg)
Cu(s) + H2O(g) is K = [H2]/[H2O].
Cu(s) + H2O(g) is K = [H2]/[H2O]. سؤال
Which reaction shown will have the highest concentration of reactants at equilibrium?
A)
B)
C)
D)
E)
A)
B)
C)
D)
E)
سؤال
Which reaction shown will have the highest concentration of products at equilibrium?
A)
B)
C)
D)
E)
A)
B)
C)
D)
E)
سؤال
Which reaction shown will have the highest concentration of reactants at equilibrium?
A)
B)
C)
D)
E)
A)
B)
C)
D)
E)
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العب
ملء الشاشة (f)
Deck 13: Equilibrium
1
Which is the correct equilibrium constant expression for the following reaction? 2C6H6(g) + 15O2(g) 12CO₂(g) + 6H₂O(g)
A)
B)
C)
D)
E)
12CO₂(g) + 6H₂O(g)A)
B)
C)
D)
E)
2
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 in order to reestablish equilibrium.
B)The reverse reaction will proceed in order 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 in order to reestablish equilibrium.
B)The reverse reaction will proceed in order to reestablish equilibrium.
C)No change occurs.
D)The equilibrium constant will increase.
E)The equilibrium constant will decrease.
The reverse reaction will proceed in order to reestablish equilibrium.
3
Write the equilibrium constant expression for the reaction shown.
A)
B)
C)
D)
E)
A)
B)
C)
D)
E)
4
The reaction system POBr3(g) POBr(g) + Br2(g) is at equilibrium.Which of the following statements describes the behavior of the system if POBr is added to the container?
A)POBr will be consumed in order to establish a new equilibrium.
B)The partial pressures of POBr3 and POBr will remain steady while the partial pressure of bromine increases.
C)The partial pressure of bromine will increase while the partial pressure of POBr decreases.
D)The partial pressure of bromine remains steady while the partial pressures of POBr3 and POBr increase.
E)The forward reaction will proceed to establish equilibrium.
POBr(g) + Br2(g) is at equilibrium.Which of the following statements describes the behavior of the system if POBr is added to the container?A)POBr will be consumed in order to establish a new equilibrium.
B)The partial pressures of POBr3 and POBr will remain steady while the partial pressure of bromine increases.
C)The partial pressure of bromine will increase while the partial pressure of POBr decreases.
D)The partial pressure of bromine remains steady while the partial pressures of POBr3 and POBr increase.
E)The forward reaction will proceed to establish equilibrium.
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5
For the reaction 2X(g) + Y(g) 2Z(g), K = 1.00 ×103 at 500 K.If at equilibrium the concentration of X is 0.20 M and the concentration of Y is 0.50 M, what is the equilibrium concentration of Z?
A)2.2 M
B)3.2 M
C)3.5 M
D)4.5 M
E)7.1 M
2Z(g), K = 1.00 ×103 at 500 K.If at equilibrium the concentration of X is 0.20 M and the concentration of Y is 0.50 M, what is the equilibrium concentration of Z?A)2.2 M
B)3.2 M
C)3.5 M
D)4.5 M
E)7.1 M
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6
What is defined as a fraction with equilibrium product concentrations in the numerator and equilibrium reactant concentrations in the denominator and each concentration raised to a power equal to the corresponding stoichiometric coefficient in the balanced chemical equation?
A)Reversibility expression
B)Reaction expression
C)Equilibrium expression
D)Product quotient
E)Mass action
A)Reversibility expression
B)Reaction expression
C)Equilibrium expression
D)Product quotient
E)Mass action
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7
Write the equilibrium constant expression for the reaction shown. 2NOCl(g) ⇌ 2NO(g) + Cl2(g)
A)
B)
C)
D)
E)
A)
B)
C)
D)
E)
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8
At equilibrium, the rate of the forward reaction is equal to the rate of the reverse reaction.
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9
Hydrogen peroxide may decompose to form water and oxygen gas according to the following reaction. 2H2O2(g) 2H2O(g) + O2(g)
In a particular experiment, 1.75 moles of H2O2 were placed in a 2.5-L reaction chamber at 307ºC.After equilibrium was reached, 1.20 moles of H2O2 remained.What is K for the reaction?
A)2.0 × 10−4
B)2.3 × 10−2
C)2.4 × 10-3
D)5.5 × 10−3
E)3.9 × 10−4
2H2O(g) + O2(g)In a particular experiment, 1.75 moles of H2O2 were placed in a 2.5-L reaction chamber at 307ºC.After equilibrium was reached, 1.20 moles of H2O2 remained.What is K for the reaction?
A)2.0 × 10−4
B)2.3 × 10−2
C)2.4 × 10-3
D)5.5 × 10−3
E)3.9 × 10−4
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10
At 35ºC, the equilibrium constant for the reaction 2NOCl(g) 2NO(g) + Cl2(g) is K = 1.6 × 10−5.An equilibrium mixture was found to have the following concentrations of Cl2 and NOCl: [Cl2] = 1.2 × 10−2 M; [NOCl] = 2.8 × 10−1 M.Calculate the concentration of NO(g) at equilibrium.
A)1.0 × 10−4 M
B)1.0 × 10−2 M
C)2.8 × 10−1 M
D)2.4 × 10−2 M
E)1.6 × 10−3 M
2NO(g) + Cl2(g) is K = 1.6 × 10−5.An equilibrium mixture was found to have the following concentrations of Cl2 and NOCl: [Cl2] = 1.2 × 10−2 M; [NOCl] = 2.8 × 10−1 M.Calculate the concentration of NO(g) at equilibrium.A)1.0 × 10−4 M
B)1.0 × 10−2 M
C)2.8 × 10−1 M
D)2.4 × 10−2 M
E)1.6 × 10−3 M
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11
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 K for this reaction? CO(g) + Br2(g) COBr2(g)
A)5.23
B)2.14
C)1.17
D)0.467
E)0.191
COBr2(g)A)5.23
B)2.14
C)1.17
D)0.467
E)0.191
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12
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 for this reaction?
A)0.309
B)0.601
C)1.66
D)2.25
E)3.24
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 for this reaction?A)0.309
B)0.601
C)1.66
D)2.25
E)3.24
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13
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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14
For the nitrogen fixation reaction, 3H2(g) + N2(g) 2NH3(g), K = 6.0 × 10−2 at 500°C.If 0.250 M H2 and 0.050 M NH3 are present at equilibrium, what is the equilibrium concentration of N2?
A)3.3 M
B)2.7 M
C)0.20 M
D)0.083 M
E)0.058 M
2NH3(g), K = 6.0 × 10−2 at 500°C.If 0.250 M H2 and 0.050 M NH3 are present at equilibrium, what is the equilibrium concentration of N2?A)3.3 M
B)2.7 M
C)0.20 M
D)0.083 M
E)0.058 M
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15
At elevated temperatures, hydrogen iodide may decompose to form hydrogen gas and iodine gas, as follows. 2HI(g) H2(g) + I2(g)
In a particular experiment, the concentrations at equilibrium were measured to be [HI] = 0.85 mol/L, [I2] = 0.60 mol/L, and [H2] = 0.27 mol/L.What is K for the above reaction?
A)5.3
B)0.22
C)4.5
D)0.19
E)1.6× 102
H2(g) + I2(g)In a particular experiment, the concentrations at equilibrium were measured to be [HI] = 0.85 mol/L, [I2] = 0.60 mol/L, and [H2] = 0.27 mol/L.What is K for the above reaction?
A)5.3
B)0.22
C)4.5
D)0.19
E)1.6× 102
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16
If, in a particular process, reactants are able to form products, and products are also able to form reactants, then this process may be described as
A)a reversible process.
B)an elementary process.
C)at equilibrium.
D)forbidden.
E)a forward process.
A)a reversible process.
B)an elementary process.
C)at equilibrium.
D)forbidden.
E)a forward process.
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17
During a chemical reaction, what defines when the concentrations of the reactants and products reach a constant level?
A)Elementary process
B)Reversible reaction
C)Rate law
D)Rate constant
E)Equilibrium
A)Elementary process
B)Reversible reaction
C)Rate law
D)Rate constant
E)Equilibrium
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18
A 6.0-L vessel was found to contain 1.0 mol BrCl3, 2.0 mol Br2 and 6.0 mol Cl2.What is the equilibrium constant, K, for this equilibrium mixture for the reaction 2BrCl3(g) Br2(g) + 3Cl2(g)?
A)0.014
B)108
C)18
D)12
E)432
Br2(g) + 3Cl2(g)?A)0.014
B)108
C)18
D)12
E)432
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19
Which substances are included in the equilibrium constant expression, Kc?
A)Only pure solids
B)Only pure liquids
C)Only pure solids and liquids
D)Only gases and dissolved substances
E)All participating substances
A)Only pure solids
B)Only pure liquids
C)Only pure solids and liquids
D)Only gases and dissolved substances
E)All participating substances
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20
Which is the correct equilibrium constant expression for the following reaction? 2BrCl3(g) Br2(g) + 3Cl2(g)
A) Kc = [Br2] [Cl2]/[BrCl3]
B) Kc = [Br2] [Cl2]5/[BrCl3]2
C) Kc = [Br2] [Cl2]3/[BrCl3]2
D) Kc = [BrCl3]2/([Br2] × [Cl2]3)
E) Kc = 2[BrCl3]2/([Br2] × 3[Cl2]3)
Br2(g) + 3Cl2(g) A) Kc = [Br2] [Cl2]/[BrCl3]
B) Kc = [Br2] [Cl2]5/[BrCl3]2
C) Kc = [Br2] [Cl2]3/[BrCl3]2
D) Kc = [BrCl3]2/([Br2] × [Cl2]3)
E) Kc = 2[BrCl3]2/([Br2] × 3[Cl2]3)
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21
When the following reaction is at equilibrium 2NOCl(g) 2NO(g) + Cl2(g)
then [NO]2 [Cl2] = K [NOCl]2.
2NO(g) + Cl2(g)then [NO]2 [Cl2] = K [NOCl]2.
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22
Which reaction shown will have the highest concentration of products at equilibrium?
A)
B)
C)
D)
E)
A)
B)
C)
D)
E)
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23
Determine the balanced chemical equation that corresponds to the given equilibrium expression.
A)
B)
C)
D)
E)
A)
B)
C)
D)
E)
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24
If the system 3H2(g) + N2(g) 2NH3(g) is at equilibrium and more N2 is added, a net reaction that consumes some of the added N2 will occur until a new equilibrium is reached.
2NH3(g) is at equilibrium and more N2 is added, a net reaction that consumes some of the added N2 will occur until a new equilibrium is reached. فتح الحزمة
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25
When a reaction system reaches equilibrium, the forward and reverse reactions stop.
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26
Determine the balanced chemical equation that corresponds to the given equilibrium expression.
A)
B)
C)
D)
E)
A)
B)
C)
D)
E)
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27
The equilibrium constant expression for the reaction CuO(s) + H2(g) Cu(s) + H2O(g) is K = [H2]/[H2O].
Cu(s) + H2O(g) is K = [H2]/[H2O]. فتح الحزمة
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28
Which reaction shown will have the highest concentration of reactants at equilibrium?
A)
B)
C)
D)
E)
A)
B)
C)
D)
E)
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29
Which reaction shown will have the highest concentration of products at equilibrium?
A)
B)
C)
D)
E)
A)
B)
C)
D)
E)
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30
Which reaction shown will have the highest concentration of reactants at equilibrium?
A)
B)
C)
D)
E)
A)
B)
C)
D)
E)
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