Chapter 6, Problem 6.36NP

(a)

Interpretation Introduction

Interpretation:

Whether the equilibrium position will shift toward reactants or products as pressure is increased should be predicted.

Concept Introduction :

Le Chatelier’s principle states that if a change in pressure, temperature or concentration takes place in an equilibrium system, the equilibrium will shift to counteract the effect of that change.

(b)

Interpretation Introduction

Interpretation:

Whether the equilibrium position will shift toward reactants or products as temperature is increased should be predicted.

Concept Introduction :

Le Chatelier’s principle states that if a change in pressure, temperature or concentration happened in an equilibrium system, the equilibrium will shift to counteract the effect of that change.

(c)

Interpretation Introduction

Interpretation:

The K_p at 600 and 700 K should be calculated.

Concept Introduction :

Clausius-Clapeyron equation is represented as follows:

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

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

(d)

Interpretation Introduction

Interpretation:

The value of K_x at 600 K and pressures 1.00 and 2.25 bar should be calculated.

Concept Introduction:

The relation between equilibrium constant in terms of concentration and pressure is represented as follows:

  $K_x=K_p.{\left(\frac{P}{P^0}\right)}^{-\Delta v}$

Here,

K_x − equilibrium constant in terms of concentrations

K_p − equilibrium constant in terms of pressure

P − total pressure

  $\Delta v=\text{ number of moles of products - number of moles of reactants}$