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In thermal physics and thermodynamics, the heat capacity ratio, also known as the adiabatic index, the ratio of specific heats, or Laplace's coefficient, is the ratio of the heat capacity at constant pressure (C P) to heat capacity at constant volume (C V).
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 specific heat ratio, (or ), is a function of only and is greater than unity. An ideal gas with specific heats independent of temperature, and , is referred to as a perfect gas . For example, monatomic gases and diatomic gases at ordinary temperatures are considered perfect gases.
The symbol c stands for the specific heat (also called “specific heat capacity”) and depends on the material and phase. The specific heat is numerically equal to the amount of heat necessary to change the temperature of \(1.00 \, kg\) of mass by \(1.00^oC\). The SI unit for specific heat is \(J/(kg \times K)\) or \(J/(kg \times ^oC)\).
The Ratio of Specific Heat is dimensionless and the value is the same in the SI and the Imperial system of units.
The SI unit for specific heat capacity is joule per kelvin per kilogram J kg⋅K , J⋅K −1 ⋅kg −1. Since an increment of temperature of one degree Celsius is the same as an increment of one kelvin, that is the same as joule per degree Celsius per kilogram: 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.
