Chapter 12, Problem 12.47SP

(a)

Interpretation Introduction

Interpretation:

The rate law for the given reaction has to be given.

Concept introduction:

Rate law:

It is an equation that related to the dependence of the reaction rate on the concentration of each substrates (reactants).  It is also said to be as rate equation.

$\begin{array}{l}\text{For}\text{a}\text{reaction}\\ \\ \text{aA}\text{+}\text{bB}\stackrel{}{\to }\text{Products}\\ \\ \text{A}\text{and}\text{B}\text{are}\text{reactants}\text{and}\text{a}\text{and}\text{b}\text{are}\text{stoichiometric}\text{coefficients}\text{.}\\ \\ \text{Rate}\text{=}\text{-}\frac{\text{Δ}\left[\text{A}\right]}{\text{Δt}}\text{=}\text{k}{\left[\text{A}\right]}^{\text{m}}{\left[\text{B}\right]}^{\text{n}}\\ \\ \text{where,}\text{k}\text{-}\text{rate}\text{constant}\text{.}\end{array}$

(b)

Interpretation Introduction

Interpretation:

The overall order of the given reaction has to be given.

Concept introduction:

Order of a reaction:

Order of a reaction is defined as the sum of exponents of the concentrations in the rate law of the given reaction.

(c)

Interpretation Introduction

Interpretation:

The change in the reaction rate has to be given when the concentration of oxygen is doubled.

Concept introduction:

Rate law:

It is an equation that related to the dependence of the reaction rate on the concentration of each substrates (reactants).  It is also said to be as rate equation.

$\begin{array}{l}\text{For}\text{a}\text{reaction}\\ \\ \text{aA}\text{+}\text{bB}\stackrel{}{\to }\text{Products}\\ \\ \text{A}\text{and}\text{B}\text{are}\text{reactants}\text{and}\text{a}\text{and}\text{b}\text{are}\text{stoichiometric}\text{coefficients}\text{.}\\ \\ \text{Rate}\text{=}\text{-}\frac{\text{Δ}\left[\text{A}\right]}{\text{Δt}}\text{=}\text{k}{\left[\text{A}\right]}^{\text{m}}{\left[\text{B}\right]}^{\text{n}}\\ \\ \text{where,}\text{k}\text{-}\text{rate}\text{constant}\text{.}\end{array}$

(d)

Interpretation Introduction

Interpretation:

The change in the reaction rate has to be given when the concentration of nitric oxide is doubled and the concentration of oxygen is halved.

Concept introduction:

Rate law:

It is an equation that related to the dependence of the reaction rate on the concentration of each substrates (reactants).  It is also said to be as rate equation.

$\begin{array}{l}\text{For}\text{a}\text{reaction}\\ \\ \text{aA}\text{+}\text{bB}\stackrel{}{\to }\text{Products}\\ \\ \text{A}\text{and}\text{B}\text{are}\text{reactants}\text{and}\text{a}\text{and}\text{b}\text{are}\text{stoichiometric}\text{coefficients}\text{.}\\ \\ \text{Rate}\text{=}\text{-}\frac{\text{Δ}\left[\text{A}\right]}{\text{Δt}}\text{=}\text{k}{\left[\text{A}\right]}^{\text{m}}{\left[\text{B}\right]}^{\text{n}}\\ \\ \text{where,}\text{k}\text{-}\text{rate}\text{constant}\text{.}\end{array}$