Chapter 11, Problem 49QRT

Interpretation Introduction

Interpretation:

The temperature of a chemical reaction having activation energy of $30kJ/mol$ has to be calculated if its temperature is lowered from room temperature, in order to slow down the reaction thousand fold.

Concept Introduction:

The temperature dependence of rate constant can be explained through Arrhenius equation.

  $k=A{e}^{\frac{-E_a}{RT}}$

Where $k$ is the rate constant, $A$ is the frequency factor, $E_a$ is the activation energy, $R$ is the universal gas constant and $T$ is the temperature.

The logarithmic form of Arrhenius is given below.

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

Where, ${\text{k}}_{\text{1}}$ and ${\text{k}}_{\text{2}}$ are the rate constants at temperature ${\text{T}}_{\text{1}}$ and ${\text{T}}_{\text{2}}$ respectively.