2.56 A 1:3 mixture of CO and H2 is passed through a catalyst to produce methane at 500 K. \mathrm{CO}(\mathrm{g})+3 \mathrm{H}_{2}(\mathrm{~g})=\mathrm{CH}_{4}(\mathrm{~g})+\mathrm{H}_{2} \mathrm{O}(\mathrm{g}) How much heat is liberated in producing a

mole of methane?How does this compare with the heat obtained from burning a mole of methane at this temperature? How does the heat of combustion of CH4 compare with the heat of combustion of CO + 3H2?