Chapter 15, Problem 74E

(a)

Interpretation Introduction

Interpretation:

The reason behind the given statement of “The activation energy of a reaction depends on the overall energy change ( $\Delta E$ ) for the reaction” being false should be explained.

Concept Introduction:

Activation energy − minimum energy barrier that should be overcome for a chemical reaction to take place.

Arrhenius equation;

  $k=A{e}^{\left(\frac{{}^{-E_a}}{RT}\right)}$

  $k=\text{ rate constant}$

  $A=\text{frequency factor}$

  $E_a=\text{activation energy of the reaction}$

  $R=\text{ universal gas constant}$

  $T=\text{temperature}$

Rate law- the relationship between the reaction rate and the concentration of the reactants

(b)

Interpretation Introduction

Interpretation:

The reason behind the givenfalse statement of “The rate law for a reaction can be deduced from examination of the overall balanced equation for the reaction.” should be explained.

Concept Introduction:

Rate law- the relationship between the reaction rate and the concentration of the reactants

(c)

Interpretation Introduction

Interpretation:

The reason behind the given false statement of “Most reactions occur by one-step mechanism” should be explained.

Concept Introduction:

Activation energy − minimum energy barrier that should be overcome for a chemical reaction to take place.

Rate law- the relationship between the reaction rate and the concentration of the reactants.