Consider the combustion of liquid methanol, CH3OH(l):

(a) What is the enthalpy change for the reverse reaction?
(b) Balance the forward reaction with whole-number coefficients. What is ΔH for the reaction represented by this equation?
(c) Which is more likely to be thermodynamically favored, the forward reaction or the reverse reaction?
(d) If the reaction were written to produce H2O(g) instead of H2O(l), would you expect the magnitude of ΔH to increase, decrease, or stay the same? Explain.

Transcribed Image Text:

CH3OH) 028)CO2(g)2 H2O(0) AFI -726.5 kJ