Chapter 5, Problem 5.16E

In atmospheric chemistry, the following chemical reaction converts ${\text{SO}}_{\text{2}}$, the predominant oxide of sulfur that comes from combustion of S-containing materials, to ${\text{SO}}_3$, which can combine with ${\text{H}}_2\text{O}$ to make sulfuric acid (and thus contribute to acid rain):

${\text{SO}}_{\text{2}}\left(g\right)+\frac{1}{2}{\text{O}}_{\text{2}}\left(g\right)\rightleftharpoons {\text{ SO}}_{\text{3}}\left(l\right)$

(a) Write the expression for K for this equilibrium. (b) Calculate the value of $\Delta G^{\text{ο}}$ for this equilibrium using the ${\Delta }_{\text{f}}{G}^{\text{ο}}$ values in Appendix 2. (c) Calculate the value of K for this equilibrium. (d) If $\text{1}\text{.00 bar}$ of ${\text{SO}}_{\text{2}}$ and $\text{1}\text{.00 bar}$ of ${\text{O}}_{\text{2}}$ are enclosed in a system in the presence of some ${\text{SO}}_3$ liquid, in which direction would the reaction move?