Chapter 17, Problem 17A.6BE

Interpretation Introduction

Interpretation:

The rate law for the reaction $\text{A + 3B }\stackrel{}{\to }\text{ C + 2D}$ is ${\text{d[C]/dt = k}}_{\text{f}}{\text{[A][B][C]}}^{-1}$.  The reaction law in the terms of reaction rate $\text{ν}$ and the units of ${\text{k}}_{\text{f}}$ when the concentrations in moles per cubic decimetre has to be expressed/

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 of formation $\text{=}$ Rate of consumption

Considering a reaction:

    $\text{2A + B }\stackrel{}{\to }\text{ 3C + D}$

Then

  $\text{-}\frac{\text{1}}{\text{2}}\frac{\text{d[A]}}{\text{dt}}\text{ = -}\frac{\text{d[B]}}{\text{dt}}\text{ = }\frac{\text{1}}{\text{3}}\frac{\text{d[C]}}{\text{dt}}\text{ = }\frac{\text{d[D]}}{\text{dt}}$

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:

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

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