Chapter 7, Problem

(a)

Interpretation Introduction

Interpretation:

The energy diagram of a system with forward reaction having activation energy ${\text{E}}_{\text{act}}\text{=}\text{+}2\text{5kcal/mol}\left(\text{+105}\text{kJ/mol}\right)$ and with the reverse reaction having activation energy ${\text{E}}_{\text{act}}\text{=}\text{+}3\text{5kcal/mol}\left(\text{+146}\text{kJ/mol}\right)$ has to be sketched. The forward reaction is whether endergonic or exergonic has to be determined.

Concept Introduction:

• Activation energy: It is defined as the minimum energy required by the reacting species in order to undergo chemical reaction.
• Change in energy taking place in a reaction can be represented in a diagram called energy diagram.
• Exergonic Reaction: In a chemical reaction if the free energy is released, it is known as exergonic reaction. The free energy is released due to the losing of energy from the reactant. The value of $\Delta G$ is negative and is spontaneous where the process takes place without the influence of any external source
• Endergonic Reaction: In a chemical reaction if the free energy is absorbed, it is known as endergonic reaction. The free energy is absorbed by the reactant to form product. The value of $\Delta G$ is positive and is nonspontaneous where the process takes place by the influence of any external source

(b)

Interpretation Introduction

Interpretation:

The $\Delta G$ for the given reaction with forward reaction having activation energy ${\text{E}}_{\text{act}}\text{=}\text{+}2\text{5kcal/mol}\left(\text{+105}\text{kJ/mol}\right)$ and with the reverse reaction having activation energy ${\text{E}}_{\text{act}}\text{=}\text{+}3\text{5kcal/mol}\left(\text{+146}\text{kJ/mol}\right)$ has to be determined.

Concept Introduction:

• Activation energy: It is defined as the minimum energy required by the reacting species in order to undergo chemical reaction.
• Exergonic Reaction: In a chemical reaction if the free energy is released, it is known as exergonic reaction. The free energy is released due to the losing of energy from the reactant. The value of $\Delta G$ is negative and is spontaneous where the process takes place without the influence of any external source
• Endergonic Reaction: In a chemical reaction if the free energy is absorbed, it is known as endergonic reaction. The free energy is absorbed by the reactant to form product. The value of $\Delta G$ is positive and is nonspontaneous where the process takes place by the influence of any external source
• Free energy change $\left(\Delta G\right)$: Change in the free energy takes place while reactants convert to product. Free energy is the difference between the energy levels of reactant and product.