Chapter 15, Problem 15.142SP

Interpretation Introduction

(a)

Interpretation:

It is to be shown that thecatalyst increases the rates of both reactions by the same factor.

Concept introduction:

Arrhenius equation basically gives the dependence of the rate constant of chemical reactionat the absolute temperature $\text{T}$, pre-exponential factors, and other constants of the reaction.

$\text{K=A}{\text{.e}}^{\frac{{\text{-E}}_{\text{a}}}{\text{RT}}}$

Where, $\text{K}$ is the rate constant, $\text{A}$ is nothing but the pre-exponential factor, $\text{T}$ is the temperature in Kelvin, a constant for chemical reaction.

Interpretation Introduction

(b)

Interpretation:

It is to be shown that the catalyst does not affect the value of the equilibrium constant by using relation between ${\text{K}}_{\text{f}}$ and ${\text{K}}_{\text{r}}$.

Concept introduction:

Chemical equilibrium is simply a state in which the forward reaction equals the rate of the rate of reverse reaction.

Reaction kinetics or the chemical kinetics is basically the branch of physical chemistry which is concerned with understanding of the chemical reactions rates.