Write the expression for $K_p$ for this reaction, and state its units.
Calculate the equilibrium partial pressures of $\text{H}_2\text{S(g)}$ and $\text{H}_2\text{(g)}$.
Calculate $K_p$ at this temperature.
At $1000\,\text{K}$, the starting partial pressures of the two gases in a mixture are given below. $\text{H}_2\text{S}(g)\;200\,\text{atm}$ $\text{CH}_4(g)\;100\,\text{atm}$ The mixture is then allowed to reach equilibrium. It is observed that the equilibrium partial pressure of $\text{CS}_2(g)$ is $2\,\text{atm}$ and that of the unreacted $\text{CH}_4(g)$ is $98\,\text{atm}$.
Predict the sign of $\Delta S^\circ$ for this reaction. Explain your answer. $\text{2H}_2\text{S}(g) + \text{CH}_4(g) \rightleftharpoons \text{CS}_2(g) + 4\text{H}_2(g)$ $\Delta H^\circ = +241\,\text{kJ mol}^{-1}$
For this reaction at $1000\,\text{K}$, the free energy change, $\Delta G^\circ$, is $+51\,\text{kJ mol}^{-1}$. Calculate the value of $\Delta S^\circ$ for this reaction, stating its units.
How would $\Delta G^\circ$, and therefore the spontaneity (feasibility) of this reaction, alter as the temperature increases? Explain your answer.