Chapter 15, Problem 15.150MP

Interpretation Introduction

(a)

Interpretation:

The value of ${\text{K}}_{\text{p}}$ for the following reaction needs to be calculated:

$\left({\text{NH}}_{\text{4}}\right)\left({\text{NH}}_{\text{2}}{\text{CO}}_{\text{2}}\right)\left(\text{s}\right)\rightleftharpoons {\text{2NH}}_{\text{3}}\left(\text{g}\right){\text{+CO}}_{\text{2}}\left(\text{g}\right)$ at $\text{25°C}$

Concept introduction:

A general equilibrium reaction can be written as follows:

$aA+bB\rightleftharpoons cC+dD$

For a general reaction, the expression for K_c can be represented as follows:

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

Interpretation Introduction

(b)

Interpretation:

The change in the total quantity of ${\text{NH}}_{\text{3}}$ due to the given conditions needs to be determined.

Concept introduction:

The compound formed by hydrogen and nitrogen is known as ammonia. Its chemical or molecular formula is ${\text{NH}}_{\text{3}}$.

According to Le Chatelier’s principle, if a change in the number of moles or pressure takes place for any reaction at equilibrium, the equilibrium is shifted to contract the change. For a change in temperature, the shift in equilibrium depends on the type of reaction that is whether it is endothermic or exothermic.