Combustion Stoichiometry and Calorimetry

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.