Chapter 12, Problem 12.113CHP

(a)

Interpretation Introduction

Interpretation:

The rate law and the value of rate constant has to be determined for the given reaction.

Concept introduction:

Rate law: It is an equation that related to the dependence of the reaction rate on the concentration of each substrate (reactants).

For a reaction,

$\text{aA}\text{+}\text{bB}\stackrel{}{\to }\text{Products}$

Where,

A and B are reactants

a and b are stoichiometric coefficients

$\text{Rate}\text{=}\text{-}\frac{\text{Δ}\left[\text{A}\right]}{\text{Δt}}\text{=}\text{k}{\left[\text{A}\right]}^{\text{x}}{\left[\text{B}\right]}^{\text{y}}$

Where,

k is the rate constant

Rate constant: Rate constant is an expression used to relate the rate of a reaction to the concentration of reactants participating in the reaction.

(b)

Interpretation Introduction

Interpretation:

The initial rate has to be calculated for the given reaction when the initial concentrations $\left[{{\text{(CH}}_{\text{3}}\text{)}}_{\text{3}}\text{N}\right]=4.2\times {10}^{-2}M$$\left[Cl{O}_2\right]=3.4\times {10}^{-2}M$

Concept introduction:

Rate law: It is an equation that related to the dependence of the reaction rate on the concentration of each substrate (reactants).

For a reaction,

$\text{aA}\text{+}\text{bB}\stackrel{}{\to }\text{Products}$

Where,

A and B are reactants

a and b are stoichiometric coefficients

$\text{Rate}\text{=}\text{-}\frac{\text{Δ}\left[\text{A}\right]}{\text{Δt}}\text{=}\text{k}{\left[\text{A}\right]}^{\text{x}}{\left[\text{B}\right]}^{\text{y}}$

Where,

k is the rate constant

Rate constant: Rate constant is an expression used to relate the rate of a reaction to the concentration of reactants participating in the reaction.