specific heat capacity
(noun)Definition of specific heat capacity
The amount of heat that must be added (or removed) from a unit mass of a substance to change its temperature by one Kelvin.
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Examples of specific heat capacity in the following topics:

Specific Heat and Heat Capacity
 Derived quantities that specify heat capacity as an intensive property (i.e., independent of the size of a sample) are the molar heat capacity, which is the heat capacity per mole of a pure substance, and the specific heat capacity, often simply called specific heat, which is the heat capacity per unit mass of a material ([c]=J/(kg*K)).
 In such cases, the specific heat capacity will be a fraction of the maximum.
 As the temperature approaches absolute zero, the specific heat capacity of a system also approaches zero, due to loss of available degrees of freedom.
 So, we have: The subscript p is a reminder that the value of specific heat capacity is valid only if the transformation takes place at constant pressure.
 Copper has a specific heat capacity of 0.383 kilojoules per kilogram per kelvin (0.383 kJ kg1 K1).
 Heat capacity is the amount of energy required to change a substance's temperature by a given amount.

Real Gases
 To understand the behavior of real gases, we must take the following properties into account: compressibility variable specific heat capacity van der Waals forces nonequilibrium thermodynamic effects molecular dissociation and elementary reactions with variable composition For most applications, such a detailed analysis is unnecessary, and the ideal gas approximation can be used with reasonable accuracy.

Calculating the Standard Enthalpy Change Directly
 Because the specific heat capacity of water (4.184 J g–1 K–1) is known to high precision, a measurement of its temperature rise due to the reaction enables one to calculate the quantity of heat released.
 The resulting calorimeter constant, expressed in J K–1, is called the heat capacity of the calorimeter.
 For reactions that can be initiated by combining two solutions, the temperature rise of the solution itself can provide an approximate value of the reaction enthalpy if we assume that the heat capacity of the solution is close to that of pure water, which will be nearly true if the solutions are dilute.
 To measure a heat capacity, a warm sample is placed in the inner compartment, which is surrounded by a mixture of ice and water.
 This, combined with the heat of fusion of ice, gives the quantity of heat lost by the sample as it cools to 0°C.
 Heat released upon a reaction is equal to the standard enthalpy change if reactants and products are at equal temperature and constant pressure.