In a gas-fired power station, the energy available from the above reaction is used to convert water in a boiler from liquid water to steam, H₂O(l) → H₂O(g) ΔH = +44.0 kJ mol⁻¹ The maximum mass of water, in grams, that could be converted from liquid water to steam by the complete oxidation of one mole of methane is A - VCE - SSCE Chemistry - Question 4 - 2004 - Paper 1

We know that from the provided ΔH reaction value of 44.0 kJ, we can derive how many grams of water can be converted to steam:

The molar mass of water (H₂O) is about 18 g/mol.

Using the formula:

Mass of water (g) = (Energy available / Energy required per mole) × Molar mass

Here, we focus solely on the 44.0 kJ needed to convert water to steam:

Mass = (44.0 kJ / 44.0 kJ/mol) × 18 g/mol = 18 g

However, this mass conversion is only valid for the given energy versus the stoichiometric hold on the methane combustion, indicating we should consider the entire energy from one mole of methane combustion.

Given that each mole of methane creates enough energy to reach the maximum conversion, the final answer based on the provided options should be D. 368 grams of water can be converted to steam using this energy.