At 1 atm, how much energy is required to heat 71.0 g H2O(s) at 14.0 C to H2O(g) at 147.0 C? Use the heat transfer constants found in this table.

q=____kj

\begin{tabular}{|l|l|l|} \hline Quantity & per gram & per mole \\ \hline Enthalpy of fusion at 0C & 333.6J/g & 6010.J/mol \\ \hline Enthalpy of vaporization at 100C & 2257J/g & 40660J/mol \\ \hline Specific heat of solid H2O (ice) & 2.087J/(gC) & 37.60J/(molC) \\ \hline Specific heat of liquid H2O (water) & 4.184J/(gC) & 75.37J/(molC) \\ \hline Specific heat of gaseous H2O( steam) & 2.000J/(gC) & 36.03J/(molC) \\ \hline \end{tabular}