Chapter 12, Problem 63QAP

(a)

Interpretation Introduction

Interpretation: The number of H atoms at equilibrium needs to be determined.

Concept Introduction: The system is said to be in equilibrium if the there is no change in the partial pressure or concentration of reactant and product takes place.

For a general equilibrium reaction as follows:

  $\text{A}\left(g\right)+\text{B}\left(g\right)\rightleftharpoons \text{C}\left(g\right)+\text{D}\left(g\right)$

The expression for the equilibrium constant is represented as follows:

  $K=\frac{\left(P_C\right)\left(P_D\right)}{\left(P_A\right)\left(P_B\right)}$

Here, to calculate the equilibrium constant, the values of partial pressure of all the species in reactant and product side are required.

Ideal gas equation is as follows:

  $P=\frac{nRT}{V}$

Here, P is pressure, n is number of moles, R is Universal gas constant, T is temperature and V is volume.

In 1 mol of any substance there are $6.023\times {10}^{23}$ units.

(b)

Interpretation Introduction

Interpretation: The percent (in moles) of hydrogen gas dissociated needs to be determined.

Concept Introduction: The percent of any species dissociated in a reaction can be calculated using the following formula:

  $\%=\frac{n_{\text{dissociated}}}{n_{\text{initial}}}\times 100\%$

Here, $n_{\text{dissociated}}$ is number of moles of species dissociated and $n_{\text{initial}}$ is initial number of moles present in the solution.