Chapter 5.11, Problem 33P

(a)

Interpretation Introduction

Interpretation:

It should be determined that how increasing the experimental activation energy affects the rate constant for a reaction.

Concept introduction:

• Arrhenius equation used to find the rate constant by showing the fraction of collisions with effective orientation and represents the fraction of collisions with sufficient energy to produce a reaction.  Also this reaction gives the quantitative relation of temperature with the rate constant of reaction.

$\boxed{k=A{e}^{\frac{{}^{-E_a}}{RT}}}$

k is the rate constant, A is the frequency factor, $E_a$ is the activation energy

R is the gas constant and T is the temperature.

(b)

Interpretation Introduction

Interpretation:

It should be determined that how increasing the temperature affects the rate constant for a reaction.

Concept introduction:

• Arrhenius equation used to find the rate constant by showing the fraction of collisions with effective orientation and represents the fraction of collisions with sufficient energy to produce a reaction.  Also this reaction gives the quantitative relation of temperature with the rate constant of reaction.

$\boxed{k=A{e}^{\frac{{}^{-E_a}}{RT}}}$

k is the rate constant, A is the frequency factor, $E_a$ is the activation energy

R is the gas constant and T is the temperature.