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Joule (J): Unit of heat most commonly used in the SI system. 1.00 cal = 4.184 J. Specific Heat (cs): The quantity of heat liberated or absorbed when the temperature of 1.00 gram of a substance falls or rises 1.00 C. Specific heat is temperature (and phase) dependent.
The SI unit for specific heat is \(J/(kg \times K)\) or \(J/(kg \times ^oC)\). (Recall that the temperature change \(\Delta T\) is the same in units of kelvin and degrees Celsius.) Values of specific heat must generally be measured, because there is no simple way to calculate them precisely.
The symbol c stands for specific heat and depends on the material and phase. The specific heat is the amount of heat necessary to change the temperature of 1.00 kg of mass by 1.00ºC. The specific heat c is a property of the substance; its SI unit is J/(kg⋅K) or J/(kg⋅C).
The units of specific heat are J/(kg ⋅ °C ⋅ °C) and J/(kg ⋅ ⋅ K). However, degrees Celsius and Kelvins are not always interchangeable. The formula for specific heat uses a difference in temperature and not absolute temperature. This is the reason that degrees Celsius may be used in place of Kelvins.
Specific Heat Worksheet. DIRECTIONS: Use q = (m)(ΔT)(Cp) to solve the following problems. Show all work and units. 1. A 15.75-g piece of iron absorbs 1086.75 joules of heat energy, and its temperature changes from 25°C to 175°C. Calculate the specific heat capacity of iron. 2.
Heat capacity of crystalline solids. Heat capacity is the increment in energy required to change the temperature of some quantity of matter. Experiments show that CV depends on temperature, in general. CV ~ T3 as T → 0. Figure on right is the heat capacity of diamond.
Specific Heat of Solids. Object: To determine the specific heat of a given solid specimen. Theory: Thermal energy is an internal energy that consists of the kinetic and potential energies associated with the random motions of the atoms, molecules, and other microscopic bodies within an object.
