(a)[3]
Define, with the help of an equation that includes state symbols, the standard enthalpy change of combustion, \Delta H_c^, for methanol at $298\text{ K}$.
(b)[3]
Use these values to work out \Delta H_{\text{reaction}}^ for the synthesis of methanol, using the equation below. Include a sign in your answer. $\text{CO}(g) + 2\text{H}_2(g) \rightarrow \text{CH}_3\text{OH}(g)$ $\Delta H_{\text{reaction}}^$ = ................. $\text{kJ mol}^{-1}$
(c)[6]
The reaction is carried out under these conditions: pressure $200$ atmospheres $(2 \times 10^7\,\text{Pa})$, temperature $600\,\text{K}$, catalyst oxides of Cr, Cu, and Zn. In the spaces below, describe how each condition influences the rate at which methanol forms: pressure temperature catalyst