Chapter 16, Problem 16.53P

(a)

Interpretation Introduction

Interpretation:

The relationship between ‘k’ and time-t’ has to be graphed.

Concept introduction:

Arrhenius relation: This relation talks about the dependence of absolute temperature on the rate constant of chemical reaction.

The minimum amount of energy required for the reactants to start a chemical reaction is known as activation energy. The activation energy is represented as $\text{Ea}$.

Arrhenius equation: ${\text{k=Ae}}^{\text{-}\frac{\text{Ea}}{\text{RT}}}$

$\text{k}$ is the rate constant for the reaction.

$\text{A}$ is the Arrhenius constant.

${\text{E}}_{\text{a}}$ is the activation energy.

$\text{R}$ is universal gas constant.

$\text{T}$ is the temperature.

(b)

Interpretation Introduction

Interpretation:

The relationship between ‘ln k’ and ‘1/T’ has to be graphed; the activation energy has to be determined from the graph.

Concept introduction:

Arrhenius relation: This relation talks about the dependence of absolute temperature on the rate constant of chemical reaction.

The minimum amount of energy required for the reactants to start a chemical reaction is known as activation energy. The activation energy is represented as $\text{Ea}$.

Arrhenius equation: ${\text{k=Ae}}^{\text{-}\frac{\text{Ea}}{\text{RT}}}$

$\text{k}$ is the rate constant for the reaction.

$\text{A}$ is the Arrhenius constant.

${\text{E}}_{\text{a}}$ is the activation energy.

$\text{R}$ is universal gas constant.

$\text{T}$ is the temperature.