Using the Following Data for Water, Determine the Energy Required

Multiple Choice

Using the following data for water, determine the energy required to melt 1.00 mole of ice (solid water) at its melting point. $$\begin{array} { | l | l | } \hline \text { Boiling point } & 373 \mathrm {~K} \\\hline \text { Melting point } & 273 \mathrm {~K} \\\hline \text { Enthalpy of vaporization } & 2,260 \mathrm {~J} / \mathrm { g } \\\hline \text { Enthalpy of fusion } & 334 \mathrm {~J} / \mathrm { g } \\\hline \text { Specific heat capacity (solid) } & 2.11 \mathrm {~J} / ( \mathrm { g } \cdot \mathrm { K } ) \\\hline \text { Specific heat capacity (liquid) } & 4.18 \mathrm {~J} / ( \mathrm { g } \cdot \mathrm { K } ) \\\hline \text { Specific heat capacity (gas) } & 2.08 \mathrm {~J} / ( \mathrm { g } \cdot \mathrm { K } ) \\\hline\end{array}$$

A) 11.7 kJ
B) 23.2 kJ
C) 4.96 kJ
D) 6.02 kJ
E) 2.26 kJ