Heat Capacity is defined by Robinson and Haas (1983) as the quantity of heat that is required to raise the temperature of a unit quantity of a given substance by one degree Kelvin at a constant pressure.
A brief history of the concept
Prior to the development of the modern theories of thermodynamics, it was widely thought that heat was some form of a fluid called calorific (Cengel, 2007).Different bodies were capable of effectively holding a certain quantity of this fluid and their ability to hold such a fluid was referred to as heat capacity as was initially investigated by one Joseph Black in 1750s (Laider,1993).In this age and time, we discuss the concept of the internal energy system. This comprises of microscopic kinetic as well as potential energy. Heat too is never considered as a fluid but is regarded as a transfer of energy which is disordered at a microscopic level.
The theory of heat capacity
Heat capacity (C) a term which is otherwise referred to as thermal capacity is the physical quantity which is measurable and that characterizes the amount of heat that is required in order to change the temperature of a substance by a specific amount. In terms of the International Systems of Unites (SI), the concept of heat capacity is denoted in unites of joule(s) (J) per kelvin (K).
There are several derived quantities that are used in the specification of the concept of heat capacity as a physical quantity with intensive property. This is to say that the quantity is expressed as an independent one in regard to the sample size. These are known as molar heat capacity a concept which refers to the heat capacity per mole of a given pure substance, Specific heat capacity...
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