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The heat Q required to change the phase of a sample of mass m is given by \(\mathrm{Q=mL_f}\) (melting or freezing) and \(\mathrm{Q=mL_v}\) (evaporating or condensing), where \(\mathrm{L_f}\) and \(\mathrm{L_v}\) are the latent heat of fusion and the latent heat of vaporization, respectively.
The latent heat of fusion is the amount of heat needed to cause a phase change between solid and liquid. The latent heat of vaporization is the amount of heat needed to cause a phase change between liquid and gas.
Latent heat (also known as latent energy or heat of transformation) is energy released or absorbed, by a body or a thermodynamic system, during a constant-temperature process—usually a first-order phase transition, like melting or condensation.
The latent heat associated with melting a solid or freezing a liquid is called the latent heat of fusion ($L_{f}$); that associated with vapourizing a liquid or a solid or condensing a vapour is called the latent heat of vaporization ($L_{v}$).
Latent heat is measured in units of J/kg. Both Lf and Lv depend on the substance, particularly on the strength of its molecular forces as noted earlier. Lf and Lv are collectively called latent heat coefficients.
Latent heat is measured in units of J/kg. Both \(L_f\) and \(L_v\) depend on the substance, particularly on the strength of its molecular forces as noted earlier. \(L_f\) and \(L_v\) are collectively called latent heat coefficients.
Exothermic phase changes release heat to the environment. (They are warming processes.) The specific latent heat (L) of a material… is a measure of the heat energy (Q) per mass (m) released or absorbed during a phase change. is defined through the formula Q = mL. is often just called the "latent heat" of the material.
