Chapter 16, Problem 16.67P

Interpretation Introduction

Interpretation:

The activation energy of the given reaction has to be calculated.

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.

Activation energy for two rate constants with two different temperatures can be calculated by Arrhenius equation:

$\text{ln}\frac{{\text{k}}_{\text{2}}}{{\text{k}}_{\text{1}}}\text{=}\frac{\text{Ea}}{\text{R}}\left(\frac{\text{1}}{{\text{T}}_{\text{1}}}\text{-}\frac{\text{1}}{{\text{T}}_{\text{2}}}\right)$

$\begin{array}{l}{\text{k}}_{\text{1}}\text{,}{\text{k}}_{\text{2}}\text{=}\text{Rate}\text{constants}\\ \\ \text{Ea}\text{=}\text{Activation}\text{energy}\\ \\ \text{R}\text{=}\text{gas}\text{constant}\text{(8}\text{.314}\text{J/mol}\text{.K)}\\ \\ {\text{T}}_{\text{1}}{\text{,T}}_{\text{2}}\text{=}\text{temperatures}\end{array}$