Chapter 14, Problem 14.28QE

Interpretation Introduction

Interpretation:

The value of equilibrium constant $K_{\text{p}}$ for the following reaction has to be determined.

  ${\text{N}}_2\left(\text{g}\right)+3{\text{H}}_2\left(\text{g}\right)\rightleftharpoons 2{\text{NH}}_3\left(\text{g}\right)$

Concept Introduction:

The relation of equilibrium constant $K_{\text{p}}$ and $K_{\text{c}}$ is as follows:

  $K_{\text{p}}=K_{\text{c}}{\left(RT\right)}^{\Delta n}$        (1)

Here, $\Delta n$ is change in number of moles of gas.

The formula to calculate the value of $\Delta n$ is as follows:

  $\Delta n=\left(\begin{array}{l}\text{total number of moles of}\\ \text{gas on the product side}\end{array}\right)-\left(\begin{array}{l}\text{total number of moles of}\\ \text{gas on the reactant side}\end{array}\right)$        (2)

The value of $\Delta n$ can be zero, negative and positive.