the heat released by a unit mass of liquid to be transferred into solid at its freezing point. answer in one word please guys
Answers
Explanation:
Previously, we have discussed temperature change due to heat transfer. No temperature change occurs from heat transfer if ice melts and becomes liquid water (i.e., during a phase change). For example, consider water dripping from icicles melting on a roof warmed by the Sun. Conversely, water freezes in an ice tray cooled by lower-temperature surroundings.
Melting Icicle: Heat from the air transfers to the ice causing it to melt.
Energy is required to melt a solid because the cohesive bonds between the molecules in the solid must be broken apart so that the molecules can move around at comparable kinetic energies; thus, there is no rise in temperature. Similarly, energy is needed to vaporize a liquid, because molecules in a liquid interact with each other via attractive forces. There is no temperature change until a phase change is complete. The temperature of a glass of lemonade initially at 0 ºC stays at 0 ºC until all the ice has melted. Conversely, energy is released during freezing and condensation, usually in the form of thermal energy. Work is done by cohesive forces when molecules are brought together. The corresponding energy must be given off (dissipated) to allow them to stay together.
The energy involved in a phase change depends on two major factors: the number and strength of bonds or force pairs. The number of bonds is proportional to the number of molecules and thus to the mass of the sample. The strength of forces depends on the type of molecules. The heat Q required to change the phase of a sample of mass m is given by
[latex]\text{Q}=\text{mL}_{\text{f}}[/latex] (melting or freezing)
[latex]\text{Q}=\text{mL}_{\text{v}}[/latex] (evaporating or condensing)
where the latent heat of fusion, Lf, and latent heat of vaporization, Lv, are material constants that are determined experimentally.