Energy is absorbed or released when a material undergoes a phase transition. For example, energy is absorbed when water in its solid phase, ice, melts to form its liquid phase, liquid water.

The unusual feature is that while energy is being transferred into or out of the system during a phase change, there is no change in temperature.

The energy required varies depending on the material and the specific phase transition. This energy is expressed in terms of a latent $($or hidden$)$ heat. The latent heat of fusion for water is $3\mathrm{.}34105$J$/$kg and the latent heat of vaporization for water is $2\mathrm{.}26106$J$/$kg$.$

What is the heat $($energy$)$ required to turn a $7\mathrm{.}80-$kg block of ice at T$=0$C into $7\mathrm{.}80$kg of liquid water at T$=0$C$?$

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What is the heat $($energy$)$ released when turning $7\mathrm{.}80$kg of liquid water at T$=0$C into a $7\mathrm{.}80-$kg block of ice at T$=0$C$?$

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What is the heat $($energy$)$ required to turn $7\mathrm{.}80$kg of liquid water at T$=100$C into $7\mathrm{.}80$kg of steam at T$=100$C$?$

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What is the heat $($energy$)$ released when turning $7\mathrm{.}80$kg of steam at T$=100$C into $7\mathrm{.}80$kg of water at T$=100$C$?$