Chapter 5, Problem 35P

(a)

Interpretation Introduction

Interpretation:

Number of intermediate formed in the reaction has to be determined.

Concept introduction:

• Reaction coordinate diagram is an abstract one dimensional coordinate which represents progress along a reaction pathway.
• Reactant: These are the substances initially present in a chemical reaction. 
• Product: These are the substances produced from reactants after a successful reaction.
• Transition state: It is a hypothetical state that occurs in the space between the reactant and products in a chemical reaction.
• Intermediate: It is a molecular entity formed from the reactants and reacts further to give the products.

  The mathematical relationship between enthalpy (H) and free energy (G) is,

  ${\text{ΔG}}^{\text{0}}\text{=}{\text{ΔH}}^{\text{0}}\text{-}\text{TΔS}$

• In an exergonic reaction the products have a lower free energy than it consumes.
• In an endergonic reaction the product have a higher free energy than it consumes.

(b)

Interpretation Introduction

Interpretation:

The letter used to represent the transition states in the reaction has to be determined.

Concept introduction:

• Reaction coordinate diagram is an abstract one dimensional coordinate which represents progress along a reaction pathway.
• Reactant: These are the substances initially present in a chemical reaction. 
• Product: These are the substances produced from reactants after a successful reaction.
• Transition state: It is a hypothetical state that occurs in the space between the reactant and products in a chemical reaction.
• Intermediate: It is a molecular entity formed from the reactants and reacts further to give the products.

  The mathematical relationship between enthalpy (H) and free energy (G) is,

  ${\text{ΔG}}^{\text{0}}\text{=}{\text{ΔH}}^{\text{0}}\text{-}\text{TΔS}$

• In an exergonic reaction the products have a lower free energy than it consumes.
• In an endergonic reaction the product have a higher free energy than it consumes.

(c)

Interpretation Introduction

Interpretation:

The fastest step in the reaction has to be determined.

Concept introduction:

• Reaction coordinate diagram is an abstract one dimensional coordinate which represents progress along a reaction pathway.
• Reactant: These are the substances initially present in a chemical reaction.
• Product: These are the substances produced from reactants after a successful reaction.
• Transition state: It is a hypothetical state that occurs in the space between the reactant and products in a chemical reaction.
• Intermediate: It is a molecular entity formed from the reactants and reacts further to give the products.

  The mathematical relationship between enthalpy (H) and free energy (G) is,

  ${\text{ΔG}}^{\text{0}}\text{=}{\text{ΔH}}^{\text{0}}\text{-}\text{TΔS}$

• In an exergonic reaction the products have a lower free energy than it consumes.
• In an endergonic reaction the product have a higher free energy than it consumes.

(d)

Interpretation Introduction

Interpretation:

The more stable step has to be determined from the given steps A and G.

Concept introduction:

• Reaction coordinate diagram is an abstract one dimensional coordinate which represents progress along a reaction pathway.
• Reactant: These are the substances initially present in a chemical reaction.
• Product: These are the substances produced from reactants after a successful reaction.
• Transition state: It is a hypothetical state that occurs in the space between the reactant and products in a chemical reaction.
• Intermediate: It is a molecular entity formed from the reactants and reacts further to give the products.

  The mathematical relationship between enthalpy (H) and free energy (G) is,

  ${\text{ΔG}}^{\text{0}}\text{=}{\text{ΔH}}^{\text{0}}\text{-}\text{TΔS}$

• In an exergonic reaction the products have a lower free energy than it consumes.
• In an endergonic reaction the product have a higher free energy than it consumes.

(e)

Interpretation Introduction

Interpretation:

From the graph that whether A or E forms faster from C has to be identified.

Concept introduction:

• Reaction coordinate diagram is an abstract one dimensional coordinate which represents progress along a reaction pathway.
• Reactant: These are the substances initially present in a chemical reaction.
• Product: These are the substances produced from reactants after a successful reaction.
• Transition state: It is a hypothetical state that occurs in the space between the reactant and products in a chemical reaction.
• Intermediate: It is a molecular entity formed from the reactants and reacts further to give the products.

  The mathematical relationship between enthalpy (H) and free energy (G) is,

  ${\text{ΔG}}^{\text{0}}\text{=}{\text{ΔH}}^{\text{0}}\text{-}\text{TΔS}$

• In an exergonic reaction the products have a lower free energy than it consumes.
• In an endergonic reaction the product have a higher free energy than it consumes.

(f)

Interpretation Introduction

Interpretation:

The reactant of the rate determining step has to be identified.

Concept introduction:

• Reaction coordinate diagram is an abstract one dimensional coordinate which represents progress along a reaction pathway.
• Reactant: These are the substances initially present in a chemical reaction.
• Product: These are the substances produced from reactants after a successful reaction.
• Transition state: It is a hypothetical state that occurs in the space between the reactant and products in a chemical reaction.
• Intermediate: It is a molecular entity formed from the reactants and reacts further to give the products.

  The mathematical relationship between enthalpy (H) and free energy (G) is,

  ${\text{ΔG}}^{\text{0}}\text{=}{\text{ΔH}}^{\text{0}}\text{-}\text{TΔS}$

• In an exergonic reaction the products have a lower free energy than it consumes.
• In an endergonic reaction the product have a higher free energy than it consumes.

(g)

Interpretation Introduction

Interpretation:

It has to be determined that the first step in the reaction is whether exergonic or endergonic.

Concept introduction:

• Reaction coordinate diagram is an abstract one dimensional coordinate which represents progress along a reaction pathway.
• Reactant: These are the substances initially present in a chemical reaction.
• Product: These are the substances produced from reactants after a successful reaction.
• Transition state: It is a hypothetical state that occurs in the space between the reactant and products in a chemical reaction.
• Intermediate: It is a molecular entity formed from the reactants and reacts further to give the products.

  The mathematical relationship between enthalpy (H) and free energy (G) is,

  ${\text{ΔG}}^{\text{0}}\text{=}{\text{ΔH}}^{\text{0}}\text{-}\text{TΔS}$

• In an exergonic reaction the products have a lower free energy than it consumes.
• In an endergonic reaction the product have a higher free energy than it consumes.

(i)

Interpretation Introduction

Interpretation:

The more stable intermediate has to be determined.

Concept introduction:

• Reaction coordinate diagram is an abstract one dimensional coordinate which represents progress along a reaction pathway.
• Reactant: These are the substances initially present in a chemical reaction.
• Product: These are the substances produced from reactants after a successful reaction.
• Transition state: It is a hypothetical state that occurs in the space between the reactant and products in a chemical reaction.
• Intermediate: It is a molecular entity formed from the reactants and reacts further to give the products.

  The mathematical relationship between enthalpy (H) and free energy (G) is,

  ${\text{ΔG}}^{\text{0}}\text{=}{\text{ΔH}}^{\text{0}}\text{-}\text{TΔS}$

• In an exergonic reaction the products have a lower free energy than it consumes.
• In an endergonic reaction the product have a higher free energy than it consumes.

(j)

Interpretation Introduction

Interpretation:

It has to be identified that the step in the forward direction which has the largest rate constant.

Concept introduction:

• Reaction coordinate diagram is an abstract one dimensional coordinate which represents progress along a reaction pathway.
• Reactant: These are the substances initially present in a chemical reaction.
• Product: These are the substances produced from reactants after a successful reaction.
• Transition state: It is a hypothetical state that occurs in the space between the reactant and products in a chemical reaction.
• Intermediate: It is a molecular entity formed from the reactants and reacts further to give the products.

  The mathematical relationship between enthalpy (H) and free energy (G) is,

  ${\text{ΔG}}^{\text{0}}\text{=}{\text{ΔH}}^{\text{0}}\text{-}\text{TΔS}$

• In an exergonic reaction the products have a lower free energy than it consumes.
• In an endergonic reaction the product have a higher free energy than it consumes.
• According to rate law the rate of a reaction is directly proportional to the concentration of the reactants involved in the reaction.

  $\begin{array}{l}\text{Rate}\text{α}\left[\text{Reactants}\right]\\ \text{Rate}\text{=}\text{k}\text{×}\left[\text{Reactants}\right]\end{array}$

  Rate constant is a proportionality constant that appears in rate law. and it is independent of concentration but depend on other factors, most notably temperature.

• Forward reaction: The reaction in which the reactant that converted into product.
• Backward reaction: The reaction in which the product that converted into reactant

(k)

Interpretation Introduction

Interpretation:

It has to be identified that the step in the reverse direction which has the smallest rate constant.

Concept introduction:

• Reaction coordinate diagram is an abstract one dimensional coordinate which represents progress along a reaction pathway.
• Reactant: These are the substances initially present in a chemical reaction.
• Product: These are the substances produced from reactants after a successful reaction.
• Transition state: It is a hypothetical state that occurs in the space between the reactant and products in a chemical reaction.
• Intermediate: It is a molecular entity formed from the reactants and reacts further to give the products.

  The mathematical relationship between enthalpy (H) and free energy (G) is,

  ${\text{ΔG}}^{\text{0}}\text{=}{\text{ΔH}}^{\text{0}}\text{-}\text{TΔS}$

• In an exergonic reaction the products have a lower free energy than it consumes.
• In an endergonic reaction the product have a higher free energy than it consumes.
• According to rate law the rate of a reaction is directly proportional to the concentration of the reactants involved in the reaction.

  $\begin{array}{l}\text{Rate}\text{α}\left[\text{Reactants}\right]\\ \text{Rate}\text{=}\text{k}\text{×}\left[\text{Reactants}\right]\end{array}$

  Rate constant is a proportionality constant that appears in rate law. and it is independent of concentration but depend on other factors, most notably temperature.

• Forward reaction: The reaction in which the reactant that converted into product.
• Backward reaction: The reaction in which the product that converted into reactant