Question

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Answer 1

we have to compute the amount Q_1 of heat needed to melt that quantity of ice, and the amount Q_2 of heat needed to raise the temperature of the water from zero to 100 °celsius degree, and the amount Q_3 of heat to transform all the water vapor in steam at 100 degrees.
Now we have this:
\[\Large \begin{gathered}
{Q_1} = {\lambda _F}m = 79.7 \times 2 = ...kCal \hfill \\
\hfill \\
{Q_2} = {c_{{H_2}O}}m\Delta t = 1 \times 2 \times 100 = ...kCal \hfill \\
\hfill \\
{Q_3} = {\lambda _E}m = 539.2 \times 2 = ...kCal \hfill \\
\end{gathered} \]
where:
\[\Large {\lambda _F},\;{\lambda _E}\] are the latent heats of melting and vaporization of water respectively, and \[\Large {c_{{H_2}O}}\] is the specific heat of water
Finally, the requested amount Q_Total of heat is given by the subsequent formula:
\[\Large {Q_{Total}} = {Q_1} + {Q_2} + {Q_3} = ...\]
Please complete my computation

Answer 2

that's right!