Natural gas is very abundant in many Middle Eastern oil fields. However, the
costs of shipping the gas to markets in other parts of the world are high
because it is necessary to liquefy the gas, which is mainly methane and has a
boiling point at atmospheric pressure of \(-164{ }^{\circ} \mathrm{C}\). One
possible strategy is to oxidize the methane to methanol, \(\mathrm{CH}_{3}
\mathrm{OH},\) which has a boiling point of \(65^{\circ} \mathrm{C}\) and can
therefore be shipped more readily. Suppose that \(10.7 \times 10^{9}
\mathrm{ft}^{3}\) of methane at atmospheric pressure and \(25^{\circ}
\mathrm{C}\) is oxidized to methanol. (a) What volume of methanol is formed if
the density of \(\mathrm{CH}_{3} \mathrm{OH}\) is \(0.791 \mathrm{~g} /
\mathrm{mL} ?\) (b) Write balanced chemical equations for the oxidations of
methane and methanol to \(\mathrm{CO}_{2}(g)\) and \(\mathrm{H}_{2}
\mathrm{O}(l)\). Calculate the total enthalpy change for complete combustion of
the \(10.7 \times 10^{9} \mathrm{ft}^{3}\) of methane just described and for
complete combustion of the equivalent amount of methanol, as calculated in
part (a). (c) Methane, when liquefied, has a density of \(0.466 \mathrm{~g} /
\mathrm{mL} ;\) the density of methanol at \(25^{\circ} \mathrm{C}\) is \(0.791
\mathrm{~g} / \mathrm{mL}\). Compare the enthalpy change upon combustion of a
unit volume of liquid methane and liquid methanol. From the standpoint of
energy production, which substance has the higher enthalpy of combustion per
unit volume?
