1.           Consider the following redox reaction to produce methanol:
                                   2CH4(g) + O2(g) -->2CH3OH(g).
a. Calculate the change in enthalpy for the reaction at standardconditions using bond dissociation energies. See the b. appendixfor the table of bond energies.
b. Name two things that you could do to favor the formation ofmethanol by this reaction.
c. Using the value of ∆H calculated in 1a, is this an exothermicor endothermic reaction? Explain your answer.
d. Methane gas is a byproduct of oil extraction and of oilrefining. Release of the methane gas into the atmosphere, whichcontains 20% oxygen, does not result in the formation of methanol.That’s a surprising observation: Despite the fact that the reactionof methane and oxygen to produce methanol is product-favored atnormal temperatures, methanol is not formed spontaneouslywhen methane is released to the atmosphere. Suggest why no methanolis formed.
