Chapter 12, Problem 12.143MP

(a)

Interpretation Introduction

Interpretation:

The value of rate constant has to be calculated in units of ${\text{atm}}^{\text{-1}}{\text{s}}^{\text{-1}}$.

Concept introduction:

Integrated rate law for a second order reaction:

A second order reaction is defined as the reaction whose rate depends on the concentration of two reactants raised to the first power or of an only one reactant raised to the second power.

$\text{Rate}\text{=}\text{-}\frac{\text{Δ}\left[\text{A}\right]}{\text{Δt}}\text{=}\text{k}{\left[\text{A}\right]}^{\text{2}}$

Integrated rate law for a second order reaction is given below

$\begin{array}{l}\frac{\text{1}}{{\left[\text{A}\right]}_{\text{t}}}\text{=}\text{kt}\text{+}\frac{\text{1}}{{\left[\text{A}\right]}_{\text{0}}}\\ \text{where,}\\ {\left[\text{A}\right]}_{\text{0}}\text{-}\text{concentration}\text{of}\text{A}\text{at}\text{time}\text{t}\text{=}\text{0}\\ {\left[\text{A}\right]}_{\text{t}}\text{-}\text{concentration}\text{of}\text{A}\text{after}\text{time}\text{t}\\ \text{k}\text{-}\text{rate}\text{constant}\end{array}$

(b)

Interpretation Introduction

Interpretation:

The value of rate constant has to be calculated in usual units.

Concept introduction:

Integrated rate law for a second order reaction:

A second order reaction is defined as the reaction whose rate depends on the concentration of two reactants raised to the first power or of an only one reactant raised to the second power.

$\text{Rate}\text{=}\text{-}\frac{\text{Δ}\left[\text{A}\right]}{\text{Δt}}\text{=}\text{k}{\left[\text{A}\right]}^{\text{2}}$

Integrated rate law for a second order reaction is given below

$\begin{array}{l}\frac{\text{1}}{{\left[\text{A}\right]}_{\text{t}}}\text{=}\text{kt}\text{+}\frac{\text{1}}{{\left[\text{A}\right]}_{\text{0}}}\\ \text{where,}\\ {\left[\text{A}\right]}_{\text{0}}\text{-}\text{concentration}\text{of}\text{A}\text{at}\text{time}\text{t}\text{=}\text{0}\\ {\left[\text{A}\right]}_{\text{t}}\text{-}\text{concentration}\text{of}\text{A}\text{after}\text{time}\text{t}\\ \text{k}\text{-}\text{rate}\text{constant}\end{array}$

(c)

Interpretation Introduction

Interpretation:

After the given reaction time, the total amount of heat liberated has to be calculated when the volume of the reaction mixture is $1.00\text{ L}$

Concept introduction:

Standard enthalpy of reaction:

The change in enthalpy that is associated with the formation of one mole of a substance from its related elements being in standard state is called standard enthalpy of formation (${\text{ΔH}}_{\text{f}}\text{°}$).  The standard enthalpy of formation is used to determine the standard enthalpies of compound and element.

The standard enthalpy of reaction is the enthalpy of reaction that takes place under standard conditions.

The equation for determining the standard enthalpies of compound and element can be given by,

${\text{ΔH°}}_{\text{reaction}}\text{=}{\displaystyle \sum {\text{nΔH°}}_{\text{f}}\text{(products)}}\text{-}{\displaystyle \sum {\text{mΔH°}}_{\text{f}}\text{(reactants)}}$