(a) Given ΔH° for the reaction

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 H° for its hydrogenation to ethylene? To ethane?
(c) What is the value of ΔH° for the hypothetical reaction
2CH2==CH2(g) -†’ CH3CH3(g) + HC‰¡‰¡CH(g)

Transcribed Image Text:

H2(g) + 0,(g) → H,0(1) AH° -286 kJ