## College Physics (4th Edition)

$56,900~J$ of heat are required.
We can find the number of moles of hydrogen: $PV = nRT$ $n = \frac{PV}{RT}$ $n = \frac{(10.0)(1.013\times 10^5~Pa)(250\times 10^{-3}~m^3)}{(8.314~J/mol~K)(273.15~K)}$ $n = 111.5~mol$ We can find the required heat: $Q = c~n~\Delta T$ $Q = (20.4~J/mol~K)(111.5~mol)(25.0~K)$ $Q = 56,900~J$ $56,900~J$ of heat are required.