Problem: Part A. What volume of methanol is formed if 2.94×1011 L of methane at standard atmospheric pressure and 25°C is oxidized to methanol? The density of CH3OH is 0.791 g/ mL. Assume that the oxidation of methane to methanol occurs in a 1:1 stoichiometry.Natural gas (mostly methane, CH4) 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 has a boiling point of − 164°C. One possible strategy is to oxidize the methane (in a 1:1 mole ratio) to methanol, CH3OH, which has a boiling point of 65°C and can therefore be shipped more readily.

Problem Details

Part A. What volume of methanol is formed if 2.94×1011 L of methane at standard atmospheric pressure and 25°C is oxidized to methanol? The density of CH3OH is 0.791 g/ mL.

Assume that the oxidation of methane to methanol occurs in a 1:1 stoichiometry.

Natural gas (mostly methane, CH4) 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 has a boiling point of − 164°C. One possible strategy is to oxidize the methane (in a 1:1 mole ratio) to methanol, CH3OH, which has a boiling point of 65°C and can therefore be shipped more readily.