Chapter 6, Problem 6.43P

Interpretation Introduction

(a)

Interpretation: The points on the graph correspond to transition states are to be identified.

Concept introduction: The transition state is formed during the conversion of reactants into products in the chemical reaction. In an energy level diagram, it corresponds to the high potential energy along the y-axis. In this state, the dashed bond implies that bonds are partially broken and partially formed in the reaction.

Interpretation Introduction

(b)

Interpretation: The points that correspond to reactive intermediates are to be stated.

Concept introduction: The transition state is formed during the conversion of reactants into products in the chemical reaction. In an energy level diagram, it corresponds to the high potential energy along the y-axis, while reactive intermediate has low potential energy.

Interpretation Introduction

(c)

Interpretation: The number of steps present in the reaction mechanism is to be identified.

Concept introduction: The number of steps in the reaction depends on the mechanism of the reaction. The activation energy $\left(E_{\text{a}}\right)$ aids in determining the rate of the chemical reactions. The small value of $E_{\text{a}}$ exhibits that less energy is required to convert the reactants into products. It increases the rate of reaction.

Interpretation Introduction

(d)

Interpretation: The each step of the mechanism is to be labeled as endothermic or exothermic.

Concept introduction: The chemical reaction in which energy is released during the formation of products is known as exothermic reactions. The energy released during the reaction is denoted by $\Delta H°$. Exothermic and endothermic reactions are opposite to each other. The value of $\Delta H°$ for exothermic and endothermic reactions is positive and negative respectively.

Interpretation Introduction

(e)

Interpretation: The overall reaction as endothermic or exothermic is to be labeled.

Concept introduction: The chemical reaction in which energy is released during the formation of products is known as exothermic reactions. The energy released during the reaction is denoted by $\Delta H°$. Exothermic and endothermic reactions are opposite to each other. The value of $\Delta H°$ for exothermic and endothermic reactions is positive and negative respectively.