State the expression for $K_p$ for this reaction, and give its units.
Calculate the equilibrium partial pressures of $\text{H}_2\text{S(g)}$ and $\text{H}_2\text{(g)}$ if initially $p(\text{H}_2\text{S}) = 200\ \text{atm}$ and $p(\text{CH}_4) = 100\ \text{atm}$, and at equilibrium $p(\text{CS}_2) = 2\ \text{atm}$ while the remaining $p(\text{CH}_4) = 98\ \text{atm}$.
Calculate the value of $K_p$ at this temperature.
Predict the sign of $\Delta S^\circ$ for this reaction. Explain your answer.
At $1000\,\text{K}$, the free energy change, $\Delta G^\circ$, for this reaction is $+51\,\text{kJ mol}^{-1}$. Calculate the value of $\Delta S^\circ$ for this reaction, and state its units.
How would the value of $\Delta G^\circ$, and therefore the spontaneity (feasibility) of this reaction, change as the temperature increases? Explain your answer.