Chapter 14, Problem 14.1P

Interpretation Introduction

To write:The equilibrium constant expression K_cfor the given reaction

  ${\text{CH}}_{3}COOH(aq)\rightleftharpoons H_{}^{+}(aq)+C{H}_{3}CO{O}_{}^{-}(aq)$

Concept Introduction:

The equilibrium constant (K_c) is defined as the ratio of the product of concentration of reaction products at equilibrium each raised to the particular stoichiometric coefficient present in balanced equation to the product of concentrations of the reactants at equilibrium each raised to their specific stoichiometric coefficient at a given temperature.

General reaction:

  $\text{C+D}\rightleftarrows \text{A+B}$

  $\begin{array}{l}{K}_c=\frac{[A][B]}{[C][D]}\\ K_p=\frac{\left(P_A\right)\left(P_B\right)}{\left(P_C\right)\left(P_D\right)}\end{array}$

Where, $\text{[A]}$and $\text{[B]}$is the concentration of products

$\text{[C]}$and $\text{[D]}$is the concentration of reactants

${\text{P}}_{\text{A}}$and ${\text{P}}_{\text{B}}$is the partial pressure of products

${\text{P}}_{\text{c}}$and ${\text{P}}_{\text{D}}$is the partial pressure of reactants

Answer to Problem 14.1P

Solution:

  $K_c=\frac{[H^{+}][C{H}_{3}CO{O}^{-}]}{[C{H}_{3}COOH]}$

Explanation of Solution

To express the equilibrium constant expression K_cfor:

  ${\text{CH}}_{3}COOH(aq)\rightleftharpoons H_{}^{+}(aq)+C{H}_{3}CO{O}_{}^{-}(aq)$

  $K_c=\frac{[H^{+}][C{H}_{3}CO{O}^{-}]}{[C{H}_{3}COOH]}$

(c)

Interpretation Introduction

To write:The equilibrium constant expression K_cfor the given reaction

  ${\text{4SO}}_3{}_{}(g)\rightleftharpoons 4S{O}_2{}_{}(g)+2O_2{}_{}(g)$

Concept Introduction:

The equilibrium constant (K_c) is defined as the ratio of the product of concentration of reaction products at equilibrium each raised to the particular stoichiometric coefficient present in balanced equation to the product of concentrations of the reactants at equilibrium each raised to their specific stoichiometric coefficient at a given temperature.

General reaction:

  $\text{C+D}\rightleftarrows \text{A+B}$

  $\begin{array}{l}{K}_c=\frac{[A][B]}{[C][D]}\\ K_p=\frac{\left(P_A\right)\left(P_B\right)}{\left(P_C\right)\left(P_D\right)}\end{array}$

Where, $\text{[A]}$and $\text{[B]}$is the concentration of products

$\text{[C]}$and $\text{[D]}$is the concentration of reactants

${\text{P}}_{\text{A}}$and ${\text{P}}_{\text{B}}$is the partial pressure of products

${\text{P}}_{\text{c}}$and ${\text{P}}_{\text{D}}$is the partial pressure of reactants

Answer to Problem 14.1P

Solution:

  $K_C=\frac{{[S{O}_2]}^4{[O_2]}^2}{{[S{O}_3]}^4}$

Explanation of Solution

To express the equilibrium constant expression K_cfor:

  ${\text{4SO}}_3{}_{}(g)\rightleftharpoons 4S{O}_2{}_{}(g)+2O_2{}_{}(g)$

  $K_C=\frac{{[S{O}_2]}^4{[O_2]}^2}{{[S{O}_3]}^4}$