The combustion of methane is represented by the equation below.
$$\mathrm{CH_4(g) + 2O_2(g) \rightarrow CO_2(g) + 2H_2O(l)}$$
The standard enthalpies of formation are provided:
$$\Delta H_f^\circ[\mathrm{CH_4(g)}] = -74.8\ \mathrm{kJ/mol}$$
$$\Delta H_f^\circ[\mathrm{CO_2(g)}] = -393.5\ \mathrmmol}$$
$$\Delta H_f^\circ[\mathrm{H_2O(l)}] = -285.8\ \mathrm{kJ/mol}$$
What volume of $$\mathrm{CH_4(g)}$$ at STP must be combusted to provide enough heat to raise the temperature of $$250\ \mathrm{g}$$ of water from $$20.0\,^{\circ}\mathrm{C}$$ to $$80.0\,^{\circ}\mathrm{C}$$? Assume the process has 100% heat transfer.