(a) Given H for the reaction H2 (g) + O2 (g) H2O (l) H = -286 kJ Along with the information that the heat

(a) Given ΔH° for the reaction
H2 (g) + ½ O2 (g) → H2O (l) ΔH° = -286 kJ
Along with the information that the heat of combustion of ethane is 1560 kJ/mol and that of ethylene is 1410 kJ/mol, calculate ΔH° for the hydrogenation of ethylene:
CH2 = CH2 (g) + H2 (g) → CH3CH3 (g)
(b) If the heat of combustion of acetylene is 1300 kJ/mol, what is the value of ΔH° for its hydrogenation to ethylene? To ethane?
(c) What is the value of ΔH° for the hypothetical reaction
2CH2 = CH2 (g) → CH3CH3 (g) _ HC + PCH (g)