Question

Consider the decomposition of liquid benzene, C₆H₆(l), to gaseous acetylene, C₂H₂(g):

C₆H₆(l) 3 C₂H₂(g) ∆H = +630 kJ

(a) What is the enthalpy change for the reverse reaction?
(b) What is ∆H for the formation of 1 mol of acetylene?
(c) Which is more likely to be thermodynamically favored, the forward reaction or the reverse reaction?
(d) If C₆H₆(g) were consumed instead of C₆H₆(l), would you expect the magnitude of ∆H to increase, decrease, or stay the same? Explain.