Chapter 13, Problem 13F.3ST

Interpretation Introduction

Interpretation:

The equilibrium constant for the dissociation process of ${\text{Na}}_{\text{2}}\left(g\right)$ at $1500\text{ K}$ has to be calculated.  Whether the corresponding answer is consistent with the statement that reaction is endothermic or not has to be stated.

Concept introduction:

The equilibrium constant of a reaction is expressed as the ratio of the partial pressure of products and reactants each raised to the power of their stoichiometric coefficients.  The formula of the equilibrium constant in term of partition function and degeneracy of the state is shown below.

    $K=\frac{g_{\text{X}}^{2}kT{\Lambda }_{{\text{X}}_{\text{2}}}^3}{g_{{\text{X}}_{\text{2}}}{p}^{\sout{\text{o}}}{q}_{{\text{X}}_{\text{2}}}^{\text{R}}{q}_{{\text{X}}_{\text{2}}}^{\text{V}}{\Lambda }_{\text{X}}^6}{\text{e}}^{-N_{A}hc{\tilde{D}}_0\left(\text{X}-\text{X}\right)/RT}$