Consider the following reaction: 2 CH3OH(g) -> 2 CH4(g) + O2 Change in Enthalpy +252.8 (a) Is this reaction exothermic or endothermic? (b) Calculate the amount of heat transferred when 24.0 g of CH3OH(g) is decomposed by this reaction at constant pressure. (c) For a given sample of CH3OH, the enthalpy change during the reaction is 82.1 kJ. How many grams of methane gas are produced? (d) How many kilojoules of heat are released when 38.5 g of CH4(g) reacts completely with O2(g) to form CH3OH(g) at constant pressure? The following is my attempt to answer the problems: (a) Endothermic (b) 24.0 g CH3OH ( 1 mole CH3OH/ 32.038 amu) = .749 moles CH3OH .749 CH3OH ( + 252.8 kJ/ 2 Moles CH3OH) = 94.67 kJ per mole of CH3OH (c) 16.039 amu/ 3.079 = 5.209 g (d) 38.5g CH4(g) ( 1mole/ 16.039 amu) = 2.4003 moles CH4 2.4003 moles CH4 (-252.8 kJ/ 2 moles CH4) = -303.397 kJ I would appreciate help with the above mentioned problems