Reaction 1 is shown below: $\text{CS}_2(g) + 3\text{O}_2(g) \rightarrow \text{CO}_2(g) + 2\text{SO}_2(g)$ Table 3.1 gives the standard enthalpy of formation, $\Delta H_f^\circ$, and the standard entropy, $S^\circ$, for some substances. Using Table 3.1, calculate the standard Gibbs free energy change, $\Delta G^\circ$, in $\text{kJ mol}^{-1}$, for reaction 1 at $25^\circ\text{C}$.
Carbon disulfide reacts with chlorine to make tetrachloromethane, as set out in reaction 2. Reaction 2: $\text{CS}_2 + 3\text{Cl}_2 \rightarrow \text{CCl}_4 + \text{S}_2\text{Cl}_2$ $\Delta H^\circ = -261.6\,\text{kJ mol}^{-1}$ $\Delta S^\circ = -365.5\,\text{J K}^{-1}\text{mol}^{-1}$ Calculate the highest temperature, in $\text{K}$, at which reaction 2 is feasible.