Chapter 17, Problem 17A.5BE

(a)

Interpretation Introduction

Interpretation:

The rate law for the reaction $\text{A + 3B }\stackrel{}{\to }\text{ C + 2D}$ was found to be ${\text{ν = k}}_{\text{f}}{\text{[A][B]}}^2$.  The units of ${\text{k}}_{\text{f}}$ has to be determined when the concentrations are in moles per cubic decimetre.

Concept Introduction:

Rate of a reaction:

Rate of a reaction is the change in concentration of reactant or product per unit time.  It is expressed in terms of decrease in concentration of any of the reactants and increase in concentration of any of the products.

Rate Law:

Rate law is experimentally determined and is used to predict the relationship between the rate of a reaction and concentration of the reactants.

For the general reaction:

    $\text{aA + bB }\stackrel{}{\to }\text{cC + dD}$

${\text{rate = k[A]}}^{\text{m}}{\text{[B]}}^{\text{n}}$

(b)

Interpretation Introduction

Interpretation:

The rate laws has to be expressed in terms of the rate of formation of C and the rate of consumption of A.

Concept Introduction:

Rate Law:

Rate law is experimentally determined and is used to predict the relationship between the rate of a reaction and concentration of the reactants.

For the general reaction:

    $\text{aA + bB }\stackrel{}{\to }\text{cC + dD}$

${\text{rate = k[A]}}^{\text{m}}{\text{[B]}}^{\text{n}}$