Chapter 6, Problem 6.4P

(a)

Interpretation Introduction

Interpretation:

Equilibrium constant $\left(\text{K}\right)$ for given reaction has to be written.

Concept introduction:

Equilibrium constant (K): In the equilibrium reaction, the ratio of concentration of the reactant and concentration of the product.  If value of K is small than 1 the reaction should be move to the left and k is more than 1 the reaction should be move to right.

Example for equilibrium reaction,

$\text{aA+bB }\stackrel{\text{K}}{\rightleftharpoons }\text{ cC+dD}$

$\text{K=}\frac{{\left[\text{C}\right]}^{\text{c}}{\left[\text{D}\right]}^{\text{d}}}{{\left[\text{A}\right]}^{\text{a}}{\left[\text{B}\right]}^{\text{b}}}$

(b)

Interpretation Introduction

Interpretation:

Equilibrium constant $\left(\text{K}\right)$ for given reaction and the pressure of a gas X as ${\text{P}}_{\text{x}}$ has to be written.

Concept introduction:

Equilibrium constant (K): In the equilibrium reaction, the ratio of concentration of the reactant and concentration of the product.  If value of K is small than 1 the reaction should be move to the left and k is more than 1 the reaction should be move to right.

Example for equilibrium reaction,

$\text{aA+bB }\stackrel{\text{K}}{\rightleftharpoons }\text{ cC+dD}$

$\text{K=}\frac{{\left[\text{C}\right]}^{\text{c}}{\left[\text{D}\right]}^{\text{d}}}{{\left[\text{A}\right]}^{\text{a}}{\left[\text{B}\right]}^{\text{b}}}$

To find pressure, the concentrations are replaced by pressure P.

$\text{K=}\frac{{\text{P}}_{\text{C}}{}^{\text{c}}{\text{.P}}_{\text{D}}{}^{\text{d}}}{{\text{P}}_{\text{A}}{}^{\text{a}}{\text{.P}}_{\text{B}}{}^{\text{b}}}$