Chapter 6, Problem 6H.1E

Interpretation Introduction

Interpretation:

From the given data the ratio of rates of catalysed to non-catalysed reactions has to be calculated.

Concept Introduction:

• Activation energy: It is defined as the minimum energy required by the reacting species in order to undergo chemical reaction.
• Activation energy can be represented as $E_a$. The unit of activation energy is $\text{kJ/mol}$.
• Catalyst: The catalyst is a chemical substance that increases the rate of the reaction without participating in the reaction by reducing the activation energy of the reaction.

Arrhenius equation:

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

$K=A{e}^{-E_a/RT}$

• $E_a$ represents the activation energy and it’s unit is kJ/mol
• R represents the universal gas constant and it has the value of $8.314J/K\times mol$
• T represents the absolute temperature
• A represents the frequency factor or collision frequency

The activation energy from the given information has to be calculated from the modified Arrhenius equation.

  $\text{ln}\frac{{\text{k}}_2}{{\text{k}}_1}\text{=}\frac{\left({\text{E}}_{{\text{a}}_{\text{1}}}{\text{-E}}_{{\text{a}}_{\text{2}}}\right)}{2.303\text{RT}}$