Chapter 7, Problem 7.64QP

Interpretation Introduction

Interpretation:

Rate law has to be written for the given reaction considering the order as $n,n\text{'}$ etc.

    ${\text{H}}_{\text{2}}\text{S}(g)+{\text{Cl}}_{\text{2}}(g)\rightleftharpoons \text{S}(s)+2\text{HCl}(g)$

Concept Introduction:

Rate of the reaction is proportional to the concentration of the reactant if all the other parameters are held as constant.  Rate of a reaction is equal to the product of rate constant and the concentration of the reactant that is raised to exponent that is reaction order.  This is termed as rate law.

Rate law for single reactant converting into product:

    $Rate=k{[A]}^n$

Where,

    $k$ is the rate constant.

    $[A]$ is the molar concentration of reactant.

    $n$ is the order of reaction.

Rate law for two reactants converting into products:

    $Rate=k{[A]}^n{[B]}^{n\text{'}}$

Where,

    $k$ is the rate constant.

    $[A],[B]$ is the molar concentration of reactant.

    $n,n\text{'}$ is the order of reaction.