Chapter 18, Problem 18.6P

Interpretation Introduction

Interpretation:

The pulse rate at ${22}^{\circ }C$ has to be calculated.

Concept Introduction:

Arrhenius relation:

This relation talks about the dependence of absolute temperature on the rate constant of chemical reaction.

The minimum amount of energy required for the reactants to start a chemical reaction is known as activation energy.  The activation energy is represented as $\text{Ea}$.

Arrhenius equation: ${\text{k = A e}}^{-\frac{\text{Ea}}{\text{RT}}}$

  $\text{k}$ is the rate constant for the reaction.

  $\text{A}$ is the Arrhenius constant.

  ${\text{E}}_{\text{a}}$ is the activation energy.

  $\text{R}$ is universal gas constant.

  $\text{T}$ is the temperature.

Activation energy for two rate constants with two different temperatures can be calculated by Arrhenius equation:

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

Where,

  ${\text{k}}_{\text{1}}\text{,}{\text{k}}_{\text{2}}$ are rate constants.

  $\text{Ea}$ is the activation energy.

  $\text{R}$ is the universal gas constant.

  ${\text{T}}_{\text{1}}{\text{,T}}_{\text{2}}$ are absolute temperatures.