Chapter 6, Problem 6.21NP

(a)

Interpretation Introduction

Interpretation:

An expression for K_p in terms of extent of reaction should be determined.

Concept Introduction :

When gases involve in a reaction, partial pressures are used instead of concentrations in the equilibrium expression.

  $\begin{array}{l}A(g)+B(g)\to C(c)+D(d)\\ K_p=\frac{P_C^c\times P_D^d}{P_A^a\times P_B^b}\end{array}$

(b)

Interpretation Introduction

Interpretation:

The expression in part (a) should be simplified limiting that x is very small.

Concept Introduction :

When gases involve in a reaction, partial pressures are used instead of concentrations in the equilibrium expression.

  $\begin{array}{l}A(g)+B(g)\to C(c)+D(d)\\ K_p=\frac{P_C^c\times P_D^d}{P_A^a\times P_B^b}\end{array}$

(c)

Interpretation Introduction

Interpretation:

The degree of dissociation of NOCl should be calculated in the limit that x is very small at $375\text{ K}$ and a pressure of $2.00\text{ bar}$

Concept Introduction :

Clausius-Clapeyron equation

  $\ln \frac{K_{P,2}}{K_{P,1}}=-\frac{\Delta H}{R}\left(\frac{1}{T_2}-\frac{1}{T_1}\right)$

  $\begin{array}{l}{K}_P\text{ - equilibrium constant}\\ \Delta H\text{ - enthalpy change}\\ \text{R - universal gas constant}\\ \text{T - temperature}\end{array}$

(d)

Interpretation Introduction

Interpretation:

The relative error in x made using the approximation in part (b) should be determined.

Concept Introduction:

  $\text{Relative error = }\frac{\text{True value - calculated value}}{\text{True value}}\times 100$