Chapter 6.5, Problem 6.8P

Consider the following reaction: ${\text{2H}}_{\text{2}}(g)+{\text{S}}_{\text{2}}(g)\stackrel{}{\rightleftarrows }{\text{2H}}_{\text{2}}\text{S}(g)$ with $K=\text{1}{\text{.1 × 10}}^{\text{7}}\text{.}$ (a) Write the expression for the equilibrium constant for this reaction. (b) Are the reactants or products favored at equilibrium? (c) Would you predict $\Delta H$ to be positive or negative? (d) Are the reactants or products lower in energy? (e) Would you predict this reaction to be fast or slow? Explain your choice.