AnswersChemistry - SC3210 A-CRLab: Reaction Rate

Reversible Reactions and Equilibrium Answers

18 verified answers2 views
1
Free Preview

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

Question illustration
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.
Option A
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.
Option B
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.
Option C
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.
Option D
2
Free Preview

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.
3

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?

Question illustration
A
2.1 x 10-2
B
2.1 x 102
C
1.2 x 103
D
1.2 x 10-3
4

Consider the reaction.At equilibrium, the concentrations of the different species are as follows.[H2O] = 0.077 M[Cl2O] = 0.077 M[HClO] = 0.023 MWhat is the equilibrium constant for the reaction at this temperature?

Question illustration
A
0.089
B
0.26
C
3.9
D
11
5

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?

Question illustration
A
1.6 ´ 10–5
B
6.2 ´ 10–4
C
6.2 ´ 104
D
1.6 ´ 105
6

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

Question illustration
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.
Option A
B
K e q equals StartFraction StartBracket upper C EndBracket StartBracket upper D EndBracket over StartBracket upper A EndBracket StartBracket upper B EndBracket EndFraction.
Option B
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.
Option C
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.
Option D
7

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?

Question illustration
A
.0059
B
5.9 x 10-2
C
0.059
D
5.9 x 102
8

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?

Question illustration
A
0.042
B
0.42
C
2.4
D
24
9

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

Question illustration
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.
10

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.
11

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

Question illustration
A
k subscript e q equals StartFraction StartBracket upper H subscript 2 upper O EndBracket over StartBracket upper H subscript 2 EndBracket StartBracket upper O subscript 2 EndBracket EndFraction.
Option A
B
k subscript e q equals StartFraction StartBracket upper H subscript 2 upper O EndBracket superscript 2 over StartBracket upper H subscript 2 EndBracket superscript 2 StartBracket upper O subscript 2 EndBracket EndFraction.
Option B
C
K subscript e q equals StartFraction StartBracket upper H subscript 2 EndBracket superscript 2 StartBracket upper O subscript 2 EndBracket over StartBracket upper H subscript 2 upper O EndBracket EndFraction.
Option C
D
K subscript e q equals StartFraction StartBracket upper H subscript 2 EndBracket superscript 2 StartBracket upper O subscript 2 EndBracket over StartBracket upper H subscript 2 upper O EndBracket superscript 2 EndFraction.
Option D
12

Consider the reaction.At equilibrium, the concentrations of the different species are as follows.[H2O] = 0.077 M[Cl2O] = 0.077 M[HClO] = 0.023 MWhat is the equilibrium constant for the reaction at this temperature?

Question illustration
A
0.089
B
0.26
C
3.9
D
11
13

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

Question illustration
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.
14

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?

Question illustration
A
0.042
B
0.42
C
2.4
D
24
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?

Question illustration
A
1.6 ´ 10–5
B
6.2 ´ 10–4
C
6.2 ´ 104
D
1.6 ´ 105
16

Consider the reaction.At equilibrium, the concentrations of the different species are as follows.[NH3] = 0.105 M[N2] = 1.1 M[H2] = 1.50 MWhat is the equilibrium constant for the reaction at this temperature?

Question illustration
A
0.0030
B
0.030
C
34
D
340
17

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?

Question illustration
A
2.1 x 10-2
B
2.1 x 102
C
1.2 x 103
D
1.2 x 10-3
18

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.
19

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
20

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.

Did you find these answers helpful?

More from this Course

Quiz
14 verified answers

Catalysts

Quiz
10 verified answers

Reaction Pathways

Quiz
10 verified answers

Reversible Reactions and Equilibrium