Chapter 6.6, Problem 7CC

 (a)

Interpretation Introduction

Interpretation:

From the given set of energy diagrams for different reactions the equilibrium, concentration of substrates involved and the more rapid reaction under given conditions should be determined.

Concept introduction:

Mechanism of the reaction is identified by using energy profile diagram; if the reaction is completed in a single step, there is only one the hump in energy diagram. Whereas if the reaction is completed in two steps there are two humps in the energy diagram, and when the Reaction is completed in multi-step there is multi hump in the energy diagram.

$\text{ΔG}$ = Gibbs free energy,

$\text{ΔG}$ (Gibbs free energy) of the reaction is mainly depends on the free energy of reactant and product. It could be positive, negative or zero depends on the number of reactant and product.

Activation energy ( $\text{Ea}$): Minimum amount of energy is needed to initiate a reaction is called activation energy.

The activation energy ( $\text{Ea}$) is calculated from the reactant energy state to the transition energy state of the reaction.

Equilibrium Constant ( $\text{Keq}$): Equilibrium Constant is the measurement of reactants which are converted in to products.

Equilibrium Constant ( $\text{Keq}$): At definite temperature, the equilibrium ratio between the product and the reactant of the reaction is called Equilibrium Constant.

$\begin{array}{l}{\text{K}}_{\text{eq}}\text{= }\frac{\left[\text{B}\right]}{\left[\text{A}\right]}\\ \text{where,}\\ \left[\text{A}\right]\text{ =}\text{Concentration of the reactant}\\ \text{[B] }\text{=}\text{Concentration of the product}\end{array}$

(b)

Interpretation Introduction

Interpretation:

From the given set of energy diagrams for different reactions the equilibrium, concentration of substrates involved and the more rapid reaction under given conditions should be determined.

Concept introduction:

Mechanism of the reaction is identified by using energy profile diagram; if the reaction is completed in a single step, there is only one the hump in energy diagram. Whereas if the reaction is completed in two steps there are two humps in the energy diagram, and when the Reaction is completed in multi-step there is multi hump in the energy diagram.

$\text{ΔG}$ = Gibbs free energy,

$\text{ΔG}$ (Gibbs free energy) of the reaction is mainly depends on the free energy of reactant and product. It could be positive, negative or zero depends on the number of reactant and product.

Activation energy ( $\text{Ea}$): Minimum amount of energy is needed to initiate a reaction is called activation energy.

The activation energy ( $\text{Ea}$) is calculated from the reactant energy state to the transition energy state of the reaction.

Equilibrium Constant ( $\text{Keq}$): Equilibrium Constant is the measurement of reactants which are converted in to products.

Equilibrium Constant ( $\text{Keq}$): At definite temperature, the equilibrium ratio between the product and the reactant of the reaction is called Equilibrium Constant.

$\begin{array}{l}{\text{K}}_{\text{eq}}\text{= }\frac{\left[\text{B}\right]}{\left[\text{A}\right]}\\ \text{where,}\\ \left[\text{A}\right]\text{ =}\text{Concentration of the reactant}\\ \text{[B] }\text{=}\text{Concentration of the product}\end{array}$

(c)

Interpretation Introduction

Interpretation:

From the given set of energy diagrams for different reactions the equilibrium, concentration of substrates involved and the more rapid reaction under given conditions should be determined.

Concept introduction:

Mechanism of the reaction is identified by using energy profile diagram; if the reaction is completed in a single step, there is only one the hump in energy diagram. Whereas if the reaction is completed in two steps there are two humps in the energy diagram, and when the Reaction is completed in multi-step there is multi hump in the energy diagram.

$\text{ΔG}$ = Gibbs free energy,

$\text{ΔG}$ (Gibbs free energy) of the reaction is mainly depends on the free energy of reactant and product. It could be positive, negative or zero depends on the number of reactant and product.

Activation energy ( $\text{Ea}$): Minimum amount of energy is needed to initiate a reaction is called activation energy.

The activation energy ( $\text{Ea}$) is calculated from the reactant energy state to the transition energy state of the reaction.

Equilibrium Constant ( $\text{Keq}$): Equilibrium Constant is the measurement of reactants which are converted in to products.

Equilibrium Constant ( $\text{Keq}$): At definite temperature, the equilibrium ratio between the product and the reactant of the reaction is called Equilibrium Constant.

$\begin{array}{l}{\text{K}}_{\text{eq}}\text{= }\frac{\left[\text{B}\right]}{\left[\text{A}\right]}\\ \text{where,}\\ \left[\text{A}\right]\text{ =}\text{Concentration of the reactant}\\ \text{[B] }\text{=}\text{Concentration of the product}\end{array}$

(d)

Interpretation Introduction

Interpretation:

From the given set of energy diagrams for different reactions the equilibrium, concentration of substrates involved and the more rapid reaction under given conditions should be determined.

Concept introduction:

Mechanism of the reaction is identified by using energy profile diagram; if the reaction is completed in a single step, there is only one the hump in energy diagram. Whereas if the reaction is completed in two steps there are two humps in the energy diagram, and when the Reaction is completed in multi-step there is multi hump in the energy diagram.

$\text{ΔG}$ = Gibbs free energy,

$\text{ΔG}$ (Gibbs free energy) of the reaction is mainly depends on the free energy of reactant and product. It could be positive, negative or zero depends on the number of reactant and product.

Activation energy ( $\text{Ea}$): Minimum amount of energy is needed to initiate a reaction is called activation energy.

The activation energy ( $\text{Ea}$) is calculated from the reactant energy state to the transition energy state of the reaction.

Equilibrium Constant ( $\text{Keq}$): Equilibrium Constant is the measurement of reactants which are converted in to products.

Equilibrium Constant ( $\text{Keq}$): At definite temperature, the equilibrium ratio between the product and the reactant of the reaction is called Equilibrium Constant.

$\begin{array}{l}{\text{K}}_{\text{eq}}\text{= }\frac{\left[\text{B}\right]}{\left[\text{A}\right]}\\ \text{where,}\\ \left[\text{A}\right]\text{ =}\text{Concentration of the reactant}\\ \text{[B] }\text{=}\text{Concentration of the product}\end{array}$

(e)

Interpretation Introduction

Interpretation:

From the given set of energy diagrams for different reactions the equilibrium, concentration of substrates involved and the more rapid reaction under given conditions should be determined.

Concept introduction:

Mechanism of the reaction is identified by using energy profile diagram; if the reaction is completed in a single step, there is only one the hump in energy diagram. Whereas if the reaction is completed in two steps there are two humps in the energy diagram, and when the Reaction is completed in multi-step there is multi hump in the energy diagram.

$\text{ΔG}$ = Gibbs free energy,

$\text{ΔG}$ (Gibbs free energy) of the reaction is mainly depends on the free energy of reactant and product. It could be positive, negative or zero depends on the number of reactant and product.

Activation energy ( $\text{Ea}$): Minimum amount of energy is needed to initiate a reaction is called activation energy.

The activation energy ( $\text{Ea}$) is calculated from the reactant energy state to the transition energy state of the reaction.

Equilibrium Constant ( $\text{Keq}$): Equilibrium Constant is the measurement of reactants which are converted in to products.

Equilibrium Constant ( $\text{Keq}$): At definite temperature, the equilibrium ratio between the product and the reactant of the reaction is called Equilibrium Constant.

$\begin{array}{l}{\text{K}}_{\text{eq}}\text{= }\frac{\left[\text{B}\right]}{\left[\text{A}\right]}\\ \text{where,}\\ \left[\text{A}\right]\text{ =}\text{Concentration of the reactant}\\ \text{[B] }\text{=}\text{Concentration of the product}\end{array}$

(f)

Interpretation Introduction

Interpretation:

From the given set of energy diagrams for different reactions the equilibrium, concentration of substrates involved and the more rapid reaction under given conditions should be determined.

Concept introduction:

Mechanism of the reaction is identified by using energy profile diagram; if the reaction is completed in a single step, there is only one the hump in energy diagram. Whereas if the reaction is completed in two steps there are two humps in the energy diagram, and when the Reaction is completed in multi-step there is multi hump in the energy diagram.

$\text{ΔG}$ = Gibbs free energy,

$\text{ΔG}$ (Gibbs free energy) of the reaction is mainly depends on the free energy of reactant and product. It could be positive, negative or zero depends on the number of reactant and product.

Activation energy ( $\text{Ea}$): Minimum amount of energy is needed to initiate a reaction is called activation energy.

The activation energy ( $\text{Ea}$) is calculated from the reactant energy state to the transition energy state of the reaction.

Equilibrium Constant ( $\text{Keq}$): Equilibrium Constant is the measurement of reactants which are converted in to products.

Equilibrium Constant ( $\text{Keq}$): At definite temperature, the equilibrium ratio between the product and the reactant of the reaction is called Equilibrium Constant.

$\begin{array}{l}{\text{K}}_{\text{eq}}\text{= }\frac{\left[\text{B}\right]}{\left[\text{A}\right]}\\ \text{where,}\\ \left[\text{A}\right]\text{ =}\text{Concentration of the reactant}\\ \text{[B] }\text{=}\text{Concentration of the product}\end{array}$

(g)

Interpretation Introduction

Interpretation:

From the given set of energy diagrams for different reactions the equilibrium, concentration of substrates involved and the more rapid reaction under given conditions should be determined.

Concept introduction:

Mechanism of the reaction is identified by using energy profile diagram; if the reaction is completed in a single step, there is only one the hump in energy diagram. Whereas if the reaction is completed in two steps there are two humps in the energy diagram, and when the Reaction is completed in multi-step there is multi hump in the energy diagram.

$\text{ΔG}$ = Gibbs free energy,

$\text{ΔG}$ (Gibbs free energy) of the reaction is mainly depends on the free energy of reactant and product. It could be positive, negative or zero depends on the number of reactant and product.

Activation energy ( $\text{Ea}$): Minimum amount of energy is needed to initiate a reaction is called activation energy.

The activation energy ( $\text{Ea}$) is calculated from the reactant energy state to the transition energy state of the reaction.

Equilibrium Constant ( $\text{Keq}$): Equilibrium Constant is the measurement of reactants which are converted in to products.

Equilibrium Constant ( $\text{Keq}$): At definite temperature, the equilibrium ratio between the product and the reactant of the reaction is called Equilibrium Constant.

$\begin{array}{l}{\text{K}}_{\text{eq}}\text{= }\frac{\left[\text{B}\right]}{\left[\text{A}\right]}\\ \text{where,}\\ \left[\text{A}\right]\text{ =}\text{Concentration of the reactant}\\ \text{[B] }\text{=}\text{Concentration of the product}\end{array}$