please answer all for thumps up

Consider the following two reactions and the corresponding enthalpy changes: CH4(g)+2O2(g)CO2(g)+2H2O(l),H1 2CH4(g)+O2(g)2CH3OH(I),H2 Given that H1=890kJ, how much heat is released or absorbed in combustion of 1 mole of methane? 890kJ released 74.80kJ released 890kJ absorbed 149.6kJ released 74.80kJ absorbed Consider the following two reactions and the corresponding enthalpy changes: CH4(g)+2O2(g)CO2(g)+2H2O(I),H12CH4(g)+O2(g)2CH3OH(I),H2 Using the heats of formation given at the beginning of the exam, determine the enthalpy change for the second reaction, H2. H2=0kJH2=163.8kJH2=327.6kJH2=163.8kJH2=327.6kJ