Reversible Reactions and Equilibrium Answers…

1

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Consider the equilibrium system below.If the system is at dynamic equilibrium, which statement is true?

A

Sublimation of the NH4CI crystals stops.

B

Solidification of the NH4CI vapors stops.

C

The rate of sublimation of the NH4CI crystals is equal to the rate of solidification of the NH4CI vapors.

D

The rate of sublimation of the NH4CI crystals is higher than the rate of solidification of the NH4CI vapors.

2

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Consider the general reversible reaction.What is the equilibrium constant expression for the given system?

A

K e q equals StartFraction lowercase C StartBracket upper C EndBracket lowercase d StartBracket upper D EndBracket over lowercase A StartBracket upper A EndBracket lowercase B StartBracket upper B EndBracket EndFraction.

B

K e q equals StartFraction StartBracket upper C EndBracket StartBracket upper D EndBracket over StartBracket upper A EndBracket StartBracket upper B EndBracket EndFraction.

C

K e q equals StartFraction StartBracket upper A EndBracket superscript lower a StartBracket upper B EndBracket superscript lower b over StartBracket upper C EndBracket superscript lower c StartBracket upper D EndBracket superscript lower D EndFraction.

D

K e q equals StartFraction StartBracket upper C EndBracket superscript lower c StartBracket upper D EndBracket superscript lower D over StartBracket upper A EndBracket superscript lower a StartBracket upper B EndBracket superscript lower b EndFraction.

3

Consider the equilibrium system below.If the system is at dynamic equilibrium, which statement is true?

A

Sublimation of the NH4CI crystals stops.

B

Solidification of the NH4CI vapors stops.

C

The rate of sublimation of the NH4CI crystals is equal to the rate of solidification of the NH4CI vapors.

D

The rate of sublimation of the NH4CI crystals is higher than the rate of solidification of the NH4CI vapors.

4

Carbon monoxide (CO) reacts with hydrogen (H2) to form methane (CH4) and water (H2O).The reaction is at equilibrium at 1,000 K. The equilibrium constant of the reaction is 3.90. At equilibrium, the concentrations are as follows.[CO] = 0.30 M[H2] = 0.10 M[H2O] = 0.020 MWhat is the equilibrium concentration of CH4 expressed in scientific notation?

A

.0059

B

5.9 x 10-2

C

0.059

D

5.9 x 102

5

Consider the reaction below.If the reaction is at dynamic equilibrium at 500 K, which statement applies to the given chemical system?

A

The forward and reverse reactions no longer occur.

B

The rates of the forward and reverse reactions are unequal.

C

The concentrations of the products and reactants do not change.

D

The forward reaction stops at 500 K.

6

Which lists all of the substances that appear in equilibrium constant expressions?

A

pure gas and pure liquid

B

pure gas and aqueous solution

C

pure solid and pure liquid

D

aqueous solution and pure liquid

7

In the atmosphere, under the effect of ultraviolet rays, oxygen molecules combine to form ozone molecules, and ozone molecules also photodissociate to form oxygen molecules. Which of the following would be observed if this reaction is in dynamic equilibrium?

A

The concentration of oxygen will increase.

B

The concentration of ozone will decrease.

C

The rates of the forward and reverse reactions will increase.

D

The rates of the forward and reverse reactions will remain the same.

8

The reaction below is at dynamic equilibrium.Which statement is true for the equilibrium system?

A

The concentration of NH3 is greater than the concentration of N2.

B

The concentration of NH3 equals the concentration of N2.

C

The rate of the forward reaction equals the rate of the reverse reaction.

D

The rate of the forward reaction is greater than the rate of the reverse reaction.

9

Consider the reaction below.At 500 K, the reaction is at equilibrium with the following concentrations.[PCI5]= 0.0095 M[PCI3] = 0.020[CI2] = 0.020 MWhat is the equilibrium constant for the given reaction?

A

0.042

B

0.42

C

2.4

D

24

10

Which represents the correct equilibrium constant expression for the reaction below?

A

K e q equals StartFraction StartBracket upper C u EndBracket StartBracket upper A g superscript plus EndBracket superscript 2 over StartBracket upper C us superscript 2 plus EndBracket StartBracket upper A g EndBracket superscript 2 EndFraction.

B

K e q equals StartFraction StartBracket upper C u superscript 2 plus EndBracket StartBracket upper A g EndBracket superscript 2 over StartBracket upper C u EndBracket StartBracket upper A g superscript plus EndBracket superscript 2 EndFraction.

C

K e q equals StartFraction StartBracket upper A g superscript plus EndBracket superscript 2 over StartBracket upper C u superscript 2 plus EndBracket EndFraction.

D

K e q equals StartFraction StartBracket upper C u superscript 2 plus EndBracket over StartBracket upper A g superscript plus EndBracket superscript 2 EndFraction.

11

Consider the reaction.At equilibrium, the concentrations are as follows.[NOCl] = 1.4 ´ 10–2 M[NO] = 1.2 ´ 10–3 M[Cl2] = 2.2 ´ 10–3 MWhat is the value of Keq for the reaction expressed in scientific notation?

A

1.6 ´ 10–5

B

6.2 ´ 10–4

C

6.2 ´ 104

D

1.6 ´ 105

12

Which statement correctly describes a reaction in dynamic equilibrium?

A

At dynamic equilibrium, the reactions stop and the amounts of reactants and products do not change.

B

At dynamic equilibrium, the reactions continue but the amounts of reactants and products do not change.

C

At dynamic equilibrium, the reactions stop but the amounts of reactants and products are changing.

D

At dynamic equilibrium, the reactions continue and the amounts of reactants and products are changing.

13

Consider the general reversible reaction.What is the equilibrium constant expression for the given system?

A

K e q equals StartFraction lowercase C StartBracket upper C EndBracket lowercase d StartBracket upper D EndBracket over lowercase A StartBracket upper A EndBracket lowercase B StartBracket upper B EndBracket EndFraction.

B

K e q equals StartFraction StartBracket upper C EndBracket StartBracket upper D EndBracket over StartBracket upper A EndBracket StartBracket upper B EndBracket EndFraction.

C

K e q equals StartFraction StartBracket upper A EndBracket superscript lower a StartBracket upper B EndBracket superscript lower b over StartBracket upper C EndBracket superscript lower c StartBracket upper D EndBracket superscript lower D EndFraction.

D

K e q equals StartFraction StartBracket upper C EndBracket superscript lower c StartBracket upper D EndBracket superscript lower D over StartBracket upper A EndBracket superscript lower a StartBracket upper B EndBracket superscript lower b EndFraction.

14

Consider the reaction.At equilibrium at 600 K, the concentrations are as follows.[HF] = 5.82 x 10-2 M[H2] = 8.4 x 10-3 M[F2] = 8.4 x 10-3 MWhat is the value of Keq for the reaction expressed in scientific notation?

A

2.1 x 10-2

B

2.1 x 102

C

1.2 x 103

D

1.2 x 10-3

15

Consider the reaction.At equilibrium, the concentrations are as follows.[NOCl] = 1.4 ´ 10–2 M[NO] = 1.2 ´ 10–3 M[Cl2] = 2.2 ´ 10–3 MWhat is the value of Keq for the reaction expressed in scientific notation?

A

1.6 ´ 10–5

B

6.2 ´ 10–4

C

6.2 ´ 104

D

1.6 ´ 105

16

Which statement correctly defines dynamic equilibrium?

A

At dynamic equilibrium, the rates of forward and reverse reactions are equal.

B

At dynamic equilibrium, the rate of the forward reaction is higher than the rate of the reverse reaction.

C

At dynamic equilibrium, the forward and reverse reactions stop.

D

At dynamic equilibrium, the concentrations of reactants and products are equal.

Reversible Reactions and Equilibrium Answers

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