🤓 Based on our data, we think this question is relevant for Professor Dunning's class at TEXAS.

** _{5}Step 1**. Determine moles of water:

$\mathbf{1}\mathbf{.}\mathbf{01}\mathbf{}\overline{)\mathbf{L}\mathbf{}{\mathbf{H}}_{\mathbf{2}}\mathbf{O}}\mathbf{\times}\frac{\mathbf{1}\mathbf{}\overline{)\mathbf{mL}}}{{\mathbf{10}}^{\mathbf{-}\mathbf{3}}\mathbf{}\overline{)\mathbf{L}}}\mathbf{\times}\frac{\mathbf{1}\mathbf{}\overline{)\mathbf{g}}}{\mathbf{1}\mathbf{}\overline{)\mathbf{mL}}}\mathbf{\times}\frac{\mathbf{1}\mathbf{}\mathbf{mol}\mathbf{}{\mathbf{H}}_{\mathbf{2}}\mathbf{O}}{\mathbf{18}\mathbf{.}\mathbf{02}\mathbf{}\overline{)\mathbf{g}\mathbf{}{\mathbf{H}}_{\mathbf{2}}\mathbf{O}}}\mathbf{=}$**56.05 mol H _{2}O **

The heat of combustion of CH_{4} is 890.4 kJ/mol and the heat capacity of H_{2}O is 75.2 J/molK.

Find the volume of methane measured at 298 K and 1.26 atm required to convert 1.01 L of water at 298 K to water vapor at 373 K.