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A piece of ice (O0C) sitting on a hot sidewalk on a hot summer day will eventually melt and then evaporate. If the ice weighs
A piece of ice (O0C) sitting on a hot sidewalk on a hot summer day will eventually melt and then evaporate. If the ice weighs 40.4 g, how much energy would be required (in kJ) to melt the ice and vaporize the ice cube?
\begin{tabular}{|c|c|} \hline TM & \begin{tabular}{l} 0.00 \\ C \end{tabular} \\ \hline TB & \begin{tabular}{l} 100.0 \\ C \end{tabular} \\ \hline \begin{tabular}{l} Specific heat \\ of liquid \\ water ( Cliquid ) \end{tabular} & \begin{tabular}{l} 4.184 \\ J/gC \end{tabular} \\ \hline \begin{tabular}{l} Enthalpy of \\ Fusion (Hfus) \end{tabular} & \begin{tabular}{l} 6.02 \\ kJ/mol \end{tabular} \\ \hline \begin{tabular}{l} Enthalpy of \\ Vaporization \\ (Hvap) \end{tabular} & \begin{tabular}{l} 40.7 \\ kJ/mol \end{tabular} \\ \hline \end{tabular}Step by Step Solution
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