For the two reactions represented by their energy profiles shown in Figure P14.1, a) Which reaction has a larger forward rate constant? b) Which reaction has a smaller reverse rate constant? c) Which reaction has a larger equilibrium constant K c ?

Question

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Answer 1

Question

Chapter 14, Problem 14.1VP

Interpretation Introduction

To find:

For the two reactions represented by their energy profiles shown in Figure P14.1,

a) Which reaction has a larger forward rate constant?

b) Which reaction has a smaller reverse rate constant?

c) Which reaction has a larger equilibrium constant K_c?

Expert Solution & Answer

Answer to Problem 14.1VP

Solution:

a) C⇌D reaction has a larger forward rate constant

b) C⇌D reaction has a smaller reverse rate constant

c) C⇌D reaction has a larger equilibrium constant K_c

Explanation of Solution

The twographs represent the energy profile diagram for the two reactions.

Reactant molecules must acquire a certain energy known as activation energy to form products. This is the different in the energies of the transition state and the reactants. For the reverse reaction, it is the difference in the energies of the transition state and the products.Maximum energy in the profile represents the transition state.

The larger the activation energy, the slower the rate of reaction.

The equilibrium constant depends on the reaction energy. If the products have less energy than the reaction, the forward reaction is favored over the reverse reaction.The value of K_eq is then larger than when reactants have less energy than the products.

a) The activation energy for the forward reaction is less in case of the second reaction, C⇌D. Therefore the forward reaction rate is larger for this reaction.

b) The activation energy for the reverse reaction is larger for the reaction C⇌D. This means the reverse reaction rate constant will be smaller for this reaction.

c) For reaction C⇌D, the product has lower energy than the reactant. For reaction A⇌B, the reactants have lower energy than the products. Therefore, reaction C⇌D will have a larger equilibrium constant KC.

Conclusion:

The energy profile of a reaction provides information about relative rates of forward and reverse rate constants as well as the relative value of the equilibrium constant.

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1. Consider these three reactions as the elementary steps in the mechanism for a chemical reaction. 2600 2400 2200 2000 1800 1600 1400 1200 1000 800 Potential Energy (kJ) 600 400 200 0 -200- -400 -600- -800 (i) Cl₂ (g) + Pt(s) → 2Cl (g) + Pt(s) (ii) Cl (g)+ CO (g) + Pt (s) → CICO (g) + Pt (s) Ea = 1550 kJ Ea = 2240 kJ (iii) Cl (g) + CICO (g) → Cl₂CO (g) Ea = 2350 kJ AH=-950 kJ ΔΗ = 575 ΚΙ AH=-825 kJ a. Draw the potential energy diagram for the reaction. Label the data points for clarity. The potential energy of the reactants is 600 kJ Reaction Progress b. What is the overall chemical equation? c. What is the overall change in enthalpy for the above chemical reaction? d. What is the overall amount of activation energy for the above chemical reaction? e. Which reaction intermediate would be considered a catalyst (if any) and why? f. If you were to add 2700kJ of energy to the reaction (e.g. 2700 kl of heat or electricity), would you be able to make the reaction reverse itself (i.e. have…

Answer 2

Question

Chapter 14, Problem 14.1VP

Interpretation Introduction

To find:

For the two reactions represented by their energy profiles shown in Figure P14.1,

a) Which reaction has a larger forward rate constant?

b) Which reaction has a smaller reverse rate constant?

c) Which reaction has a larger equilibrium constant K_c?

Expert Solution & Answer

Answer to Problem 14.1VP

Solution:

a) C⇌D reaction has a larger forward rate constant

b) C⇌D reaction has a smaller reverse rate constant

c) C⇌D reaction has a larger equilibrium constant K_c

Explanation of Solution

The twographs represent the energy profile diagram for the two reactions.

Reactant molecules must acquire a certain energy known as activation energy to form products. This is the different in the energies of the transition state and the reactants. For the reverse reaction, it is the difference in the energies of the transition state and the products.Maximum energy in the profile represents the transition state.

The larger the activation energy, the slower the rate of reaction.

The equilibrium constant depends on the reaction energy. If the products have less energy than the reaction, the forward reaction is favored over the reverse reaction.The value of K_eq is then larger than when reactants have less energy than the products.

a) The activation energy for the forward reaction is less in case of the second reaction, C⇌D. Therefore the forward reaction rate is larger for this reaction.

b) The activation energy for the reverse reaction is larger for the reaction C⇌D. This means the reverse reaction rate constant will be smaller for this reaction.

c) For reaction C⇌D, the product has lower energy than the reactant. For reaction A⇌B, the reactants have lower energy than the products. Therefore, reaction C⇌D will have a larger equilibrium constant KC.

Conclusion:

The energy profile of a reaction provides information about relative rates of forward and reverse rate constants as well as the relative value of the equilibrium constant.

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Subscribe now to access step-by-step solutions to millions of textbook problems written by subject matter experts!

Answer 3

Question

Chapter 14, Problem 14.1VP

Interpretation Introduction

To find:

For the two reactions represented by their energy profiles shown in Figure P14.1,

a) Which reaction has a larger forward rate constant?

b) Which reaction has a smaller reverse rate constant?

c) Which reaction has a larger equilibrium constant K_c?

Expert Solution & Answer

Answer to Problem 14.1VP

Solution:

a) C⇌D reaction has a larger forward rate constant

b) C⇌D reaction has a smaller reverse rate constant

c) C⇌D reaction has a larger equilibrium constant K_c

Explanation of Solution

The twographs represent the energy profile diagram for the two reactions.

Reactant molecules must acquire a certain energy known as activation energy to form products. This is the different in the energies of the transition state and the reactants. For the reverse reaction, it is the difference in the energies of the transition state and the products.Maximum energy in the profile represents the transition state.

The larger the activation energy, the slower the rate of reaction.

The equilibrium constant depends on the reaction energy. If the products have less energy than the reaction, the forward reaction is favored over the reverse reaction.The value of K_eq is then larger than when reactants have less energy than the products.

a) The activation energy for the forward reaction is less in case of the second reaction, C⇌D. Therefore the forward reaction rate is larger for this reaction.

b) The activation energy for the reverse reaction is larger for the reaction C⇌D. This means the reverse reaction rate constant will be smaller for this reaction.

c) For reaction C⇌D, the product has lower energy than the reactant. For reaction A⇌B, the reactants have lower energy than the products. Therefore, reaction C⇌D will have a larger equilibrium constant KC.

Conclusion:

The energy profile of a reaction provides information about relative rates of forward and reverse rate constants as well as the relative value of the equilibrium constant.

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Subscribe now to access step-by-step solutions to millions of textbook problems written by subject matter experts!

Answer 4

Question

Chapter 14, Problem 14.1VP

Interpretation Introduction

To find:

For the two reactions represented by their energy profiles shown in Figure P14.1,

a) Which reaction has a larger forward rate constant?

b) Which reaction has a smaller reverse rate constant?

c) Which reaction has a larger equilibrium constant K_c?

Expert Solution & Answer

Answer to Problem 14.1VP

Solution:

a) C⇌D reaction has a larger forward rate constant

b) C⇌D reaction has a smaller reverse rate constant

c) C⇌D reaction has a larger equilibrium constant K_c

Explanation of Solution

The twographs represent the energy profile diagram for the two reactions.

Reactant molecules must acquire a certain energy known as activation energy to form products. This is the different in the energies of the transition state and the reactants. For the reverse reaction, it is the difference in the energies of the transition state and the products.Maximum energy in the profile represents the transition state.

The larger the activation energy, the slower the rate of reaction.

The equilibrium constant depends on the reaction energy. If the products have less energy than the reaction, the forward reaction is favored over the reverse reaction.The value of K_eq is then larger than when reactants have less energy than the products.

a) The activation energy for the forward reaction is less in case of the second reaction, C⇌D. Therefore the forward reaction rate is larger for this reaction.

b) The activation energy for the reverse reaction is larger for the reaction C⇌D. This means the reverse reaction rate constant will be smaller for this reaction.

c) For reaction C⇌D, the product has lower energy than the reactant. For reaction A⇌B, the reactants have lower energy than the products. Therefore, reaction C⇌D will have a larger equilibrium constant KC.

Conclusion:

The energy profile of a reaction provides information about relative rates of forward and reverse rate constants as well as the relative value of the equilibrium constant.

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Subscribe now to access step-by-step solutions to millions of textbook problems written by subject matter experts!

Answer 5

Chapter 14, Problem 14.1VP

Interpretation Introduction

To find:

For the two reactions represented by their energy profiles shown in Figure P14.1,

a) Which reaction has a larger forward rate constant?

b) Which reaction has a smaller reverse rate constant?

c) Which reaction has a larger equilibrium constant K_c?

Expert Solution & Answer

Answer to Problem 14.1VP

Solution:

a) C⇌D reaction has a larger forward rate constant

b) C⇌D reaction has a smaller reverse rate constant

c) C⇌D reaction has a larger equilibrium constant K_c

Explanation of Solution

The twographs represent the energy profile diagram for the two reactions.

Reactant molecules must acquire a certain energy known as activation energy to form products. This is the different in the energies of the transition state and the reactants. For the reverse reaction, it is the difference in the energies of the transition state and the products.Maximum energy in the profile represents the transition state.

The larger the activation energy, the slower the rate of reaction.

The equilibrium constant depends on the reaction energy. If the products have less energy than the reaction, the forward reaction is favored over the reverse reaction.The value of K_eq is then larger than when reactants have less energy than the products.

a) The activation energy for the forward reaction is less in case of the second reaction, C⇌D. Therefore the forward reaction rate is larger for this reaction.

b) The activation energy for the reverse reaction is larger for the reaction C⇌D. This means the reverse reaction rate constant will be smaller for this reaction.

c) For reaction C⇌D, the product has lower energy than the reactant. For reaction A⇌B, the reactants have lower energy than the products. Therefore, reaction C⇌D will have a larger equilibrium constant KC.

Conclusion:

The energy profile of a reaction provides information about relative rates of forward and reverse rate constants as well as the relative value of the equilibrium constant.

Answer 6

Chapter 14, Problem 14.1VP

Interpretation Introduction

To find:

For the two reactions represented by their energy profiles shown in Figure P14.1,

a) Which reaction has a larger forward rate constant?

b) Which reaction has a smaller reverse rate constant?

c) Which reaction has a larger equilibrium constant K_c?

Expert Solution & Answer

Answer to Problem 14.1VP

Solution:

a) C⇌D reaction has a larger forward rate constant

b) C⇌D reaction has a smaller reverse rate constant

c) C⇌D reaction has a larger equilibrium constant K_c

Explanation of Solution

The twographs represent the energy profile diagram for the two reactions.

Reactant molecules must acquire a certain energy known as activation energy to form products. This is the different in the energies of the transition state and the reactants. For the reverse reaction, it is the difference in the energies of the transition state and the products.Maximum energy in the profile represents the transition state.

The larger the activation energy, the slower the rate of reaction.

The equilibrium constant depends on the reaction energy. If the products have less energy than the reaction, the forward reaction is favored over the reverse reaction.The value of K_eq is then larger than when reactants have less energy than the products.

a) The activation energy for the forward reaction is less in case of the second reaction, C⇌D. Therefore the forward reaction rate is larger for this reaction.

b) The activation energy for the reverse reaction is larger for the reaction C⇌D. This means the reverse reaction rate constant will be smaller for this reaction.

c) For reaction C⇌D, the product has lower energy than the reactant. For reaction A⇌B, the reactants have lower energy than the products. Therefore, reaction C⇌D will have a larger equilibrium constant KC.

Conclusion:

The energy profile of a reaction provides information about relative rates of forward and reverse rate constants as well as the relative value of the equilibrium constant.

Answer 7

Chapter 14, Problem 14.1VP

Interpretation Introduction

To find:

For the two reactions represented by their energy profiles shown in Figure P14.1,

a) Which reaction has a larger forward rate constant?

b) Which reaction has a smaller reverse rate constant?

c) Which reaction has a larger equilibrium constant K_c?

Answer 8

Expert Solution & Answer

Answer to Problem 14.1VP

Solution:

a) C⇌D reaction has a larger forward rate constant

b) C⇌D reaction has a smaller reverse rate constant

c) C⇌D reaction has a larger equilibrium constant K_c

Answer 9

Expert Solution & Answer

Answer 10

Expert Solution & Answer

Answer 11

Explanation of Solution

The twographs represent the energy profile diagram for the two reactions.

Reactant molecules must acquire a certain energy known as activation energy to form products. This is the different in the energies of the transition state and the reactants. For the reverse reaction, it is the difference in the energies of the transition state and the products.Maximum energy in the profile represents the transition state.

The larger the activation energy, the slower the rate of reaction.

The equilibrium constant depends on the reaction energy. If the products have less energy than the reaction, the forward reaction is favored over the reverse reaction.The value of K_eq is then larger than when reactants have less energy than the products.

a) The activation energy for the forward reaction is less in case of the second reaction, C⇌D. Therefore the forward reaction rate is larger for this reaction.

b) The activation energy for the reverse reaction is larger for the reaction C⇌D. This means the reverse reaction rate constant will be smaller for this reaction.

c) For reaction C⇌D, the product has lower energy than the reactant. For reaction A⇌B, the reactants have lower energy than the products. Therefore, reaction C⇌D will have a larger equilibrium constant KC.

Conclusion:

The energy profile of a reaction provides information about relative rates of forward and reverse rate constants as well as the relative value of the equilibrium constant.

Answer 12

Ch. 14 - Prob. 14.1VP Ch. 14 - Prob. 14.2VP Ch. 14 - Prob. 14.3VP Ch. 14 - Prob. 14.4VP Ch. 14 - Prob. 14.5VP Ch. 14 - Prob. 14.6VP Ch. 14 - Prob. 14.7VP Ch. 14 - Prob. 14.8VP Ch. 14 - Prob. 14.9VP Ch. 14 - Prob. 14.10VP

For the two reactions represented by their energy profiles shown in Figure P14.1, a) Which reaction has a larger forward rate constant? b) Which reaction has a smaller reverse rate constant? c) Which reaction has a larger equilibrium constant K c ?

To find: For the two reactions represented by their energy profiles shown in Figure P14.1, a) Which reaction has a larger forward rate constant? b) Which reaction has a smaller reverse rate constant? c) Which reaction has a larger equilibrium constant Kc?

Answer to Problem 14.1VP

Explanation of Solution

Want to see more full solutions like this?

Chapter 14 Solutions

To find:

For the two reactions represented by their energy profiles shown in Figure P14.1,

a) Which reaction has a larger forward rate constant?

b) Which reaction has a smaller reverse rate constant?

c) Which reaction has a larger equilibrium constant K_c?