![]() Default values will be entered for unspecified parameters. The thermodynamic property table and the graphs for water below is based on the industrial formulation by IAPWS-IF97. With specific heat c = cal/gm☌ = joule/gm☌,Ĭalculation note: Unit conversions will be performed when you enter data, but the parameters will not be forced to be consistent until you click on the quantity you wish to calculate. Heat added = specific heat x mass x ( t final - t initial)Įnter the necessary data and then click on the active text above for the quantity you wish to calculate. The amount of heat gained or lost by a sample (q) can. The heat capacity of 1 gram of a substance is called its specific heat capacity (or specific heat), while the heat capacity of 1 mole of a substance is called its molar heat capacity. The low temperature behavior is described by the Einstein-Debye model of specific heat. Heat capacity is the amount of heat required to change the temperature of a given amount of matter by 1☌. At lower temperatures the specific heats drop as quantum processes become significant. The molar specific heats of most solids at room temperature and above are nearly constant, in agreement with the Law of Dulong and Petit. For most purposes, it is more meaningful to compare the molar specific heats of substances. The specific heat per gram for water is much higher than that for a metal, as described in the water-metal example. As a result, water plays a very important role in temperature regulation. ![]() The specific heat of water is 1 calorie/gram ☌ = 4.186 joule/gram ☌ which is higher than any other common substance. The relationship does not apply if a phase change is encountered, because the heat added or removed during a phase change does not change the temperature. The relationship between heat and temperature change is usually expressed in the form shown below where c is the specific heat. The specific heat is the amount of heat per unit mass required to raise the temperature by one degree Celsius.
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