Chapter 6, Problem 6.3NP

(a)

Interpretation Introduction

Interpretation:

The value of K_p at $690\text{ K}$ should be calculated.

Concept Introduction :

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

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

Here, P is partial pressure of respective components at equilibrium.

(b)

Interpretation Introduction

Interpretation:

An equation relating K_p and the 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.

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

Here, P is partial pressure of respective components at equilibrium.

(c)

Interpretation Introduction

Interpretation:

The number of moles of each species present at equilibrium should be calculated using numerical equation solving software.

Concept Introduction :

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

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

Here, P is partial pressure of respective components at equilibrium.