Chapter 19.6, Problem 19.10WE

Interpretation Introduction

Interpretation:

For the given first order reaction with given activation energy value the rate constant for the reaction at ${\text{300}}^{\text{o}}\text{C}$ should be determined using the given rate constant for the reaction at ${\text{150}}^{\text{o}}\text{C}$.

Concept introduction:

Arrhenius equation:

• Arrhenius equation is a formula that represents the temperature dependence of reaction rates
• The Arrhenius equation has to be represented as follows

$\begin{array}{l}k=A{e}^{-E_a/RT}\\ \ln k=\ln A{e}^{-E_a/RT}\\ \ln k=\left(-\frac{{\text{E}}_{\text{a}}}{\text{R}}\right)\left(\frac{1}{\text{T}}\right)+\ln \text{A}\end{array}$

• $E_a$ represents the activation energy and it’s unit is $\text{kJ/mol}$
• R represents the universal gas constant and it has the value of 8.314 $\text{J/K}\text{.mol}$
• T represents the absolute temperature
• A represents the frequency factor or collision frequency
• e represents the base of natural logarithm
•  Arrhenius equation equation was proposed by Svante Arrhenius in 1889.