Chapter 11, Problem 72E

Interpretation Introduction

Interpretation: It is assumed by chemist that, an increase of $\text{10}\text{K}$ temperature doubles the rate of reaction. The activation energy is calculated for the given temperature to make the given statement correct.

Concept introduction: The energy difference between activated complex and reactants is known as activation energy. The relationship between the rate constant and temperature is given by the Arrhenius equation,

$k=A{e}^{\frac{-E_{\text{a}}}{RT}}$

To determine: The value of activation energy to make the statement “an increase of $\text{10}\text{K}$ temperature doubles the rate of reaction” true for a temperature increases from $\text{25}°\text{C}$ to $\text{35}°\text{C}$.