The properties c vand c p are referred to as specific heats (or heat capacities) because under certain special conditions they relate the temperature change of a system to the amount of energy added by heat transfer. Where the subscripts v and p denote the variables held fixed during differentiation. The intensive properties c v and c p are defined for pure, simple compressible substances as partial derivatives of the internal energy u(T, v) and enthalpy h(T, p), respectively: Specific heat, or specific heat capacity, is a property related to internal energy that is very important in thermodynamics. Similar definitions are associated with thermal conductivities in the y- and z-directions (ky, kz), but for an isotropic material the thermal conductivity is independent of the direction of transfer, kx = ky = kz = k.

Most materials are very nearly homogeneous, therefore we can usually write k = k (T). For vapors, it also depends upon pressure. The thermal conductivity of most liquids and solids varies with temperature. Note that Fourier’s law applies for all matter, regardless of its state (solid, liquid, or gas), therefore, it is also defined for liquids and gases. It is a measure of a substance’s ability to transfer heat through a material by conduction. The heat transfer characteristics of a solid material are measured by a property called the thermal conductivity, k (or λ), measured in W/m.K. Thermal conductivity of Water is 0.598 W/(m

For various chemical compounds and alloys, it is difficult to define the melting point, since they are usually a mixture of various chemical elements. The melting point also defines a condition in which the solid and liquid can exist in equilibrium. The melting point of a substance is the temperature at which this phase change occurs. In general, melting is a phase change of a substance from the solid to the liquid phase. Note that, these points are associated with the standard atmospheric pressure. Thermal Properties of Water Water – Melting Point

Water density