Chapter 17.6, Problem 17.14BFP

(a)

Interpretation Introduction

Interpretation:

K value at ${\text{T}}_{\text{1}}$ temperature has to be calculated.

Concept Introduction:

Equilibrium constant (K) is the equilibrium ratio of concentration/partial pressure of product to reactant in which the stoichiometric term raised to the power of each component’s concentration or partial pressure. It has a particular value at a particular temperature.

Consider a reaction, a moles of A gives b moles of B as follows,

$\text{a A }\rightleftharpoons \text{ b B}$

The equilibrium constant for this reaction can be written as follows,

$\text{K = }\frac{{\text{[B]}}_{\text{eq}}^{\text{b}}}{{\text{[A]}}_{\text{eq}}^{\text{a}}}$

Where,

    $\begin{array}{l}{\text{[A]}}_{\text{eq}}^{}\text{= equilibrium concentration of A}\\ {\text{[B]}}_{\text{eq}}^{}\text{ = equilibrium concentration of B}\\ \text{ a = stoichiometric co-efficient of A}\\ \text{ b = stoichiometric co-efficient of A}\end{array}$

(b)

Interpretation Introduction

Interpretation:

For the assumption ${\text{T}}_2<{\text{T}}_1$, sign of $\text{ΔH}$ has to be assigned for the reaction.

Concept Introduction:

During exothermic reaction energy is released. That is $\text{ΔH}$ value will be negative. Decrease in temperature favors forward reaction for exothermic processes.

During endothermic reaction heat energy is absorbed. That is $\text{ΔH}$ value will be positive. Increase in temperature favors forward reaction for endothermic processes.

(c)

Interpretation Introduction

Interpretation:

K value at ${\text{T}}_2$ temperature has to be calculated.

Concept Introduction:

Equilibrium constant (K) is the equilibrium ratio of concentration/partial pressure of product to reactant in which the stoichiometric term raised to the power of each component’s concentration or partial pressure. It has a particular value at a particular temperature.

Consider a reaction, a moles of A gives b moles of B as follows,

$\text{a A }\rightleftharpoons \text{ b B}$

The equilibrium constant for this reaction can be written as follows,

$\text{K = }\frac{{\text{[B]}}_{\text{eq}}^{\text{b}}}{{\text{[A]}}_{\text{eq}}^{\text{a}}}$

Where,

    $\begin{array}{l}{\text{[A]}}_{\text{eq}}^{}\text{= equilibrium concentration of A}\\ {\text{[B]}}_{\text{eq}}^{}\text{ = equilibrium concentration of B}\\ \text{ a = stoichiometric co-efficient of A}\\ \text{ b = stoichiometric co-efficient of A}\end{array}$