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28 Απρ 2023 · The heat capacity is a smooth, continuous function of temperature except for a small number of discontinuities. These occur at temperatures where the substance undergoes phase changes. These can be changes from one solid phase to another, melting to convert a solid phase to the liquid, or vaporization to convert the liquid to the gas.
The quantitative relationship between heat transfer and temperature change contains all three factors: Q = mcΔT, where Q is the symbol for heat transfer, m is the mass of the substance, and ΔT is the change in temperature. The symbol c stands for specific heat and depends on the material and phase.
28 Απρ 2023 · For polyatomic gases, real or ideal, CV and CP are functions of temperature. CP is always greater than CV, but as the temperature decreases, their values converge, and both vanish at absolute zero. At ordinary temperatures, CV and CP increase only slowly as temperature increases.
The heat capacity at constant volume (\(C_V\)) is defined to be the change in internal energy with respect to temperature: \[C_V = \left( \dfrac{\partial U}{\partial T} \right)_{N, V} \label{Eq3.26} \]
Define heat capacity of an ideal gas for a specific process; Calculate the specific heat of an ideal gas for either an isobaric or isochoric process; Explain the difference between the heat capacities of an ideal gas and a real gas; Estimate the change in specific heat of a gas over temperature ranges
30 Ιαν 2019 · In thermodynamics, we define heat capacity in terms of internal energy U and enthalpy H, not in terms of heat. In this way, heat capacity is a physical property of the material being processed, and not a function of the process path.
Chapter 2 Classical Thermodynamics: The Second Law. 2.1 Heat engines and refrigerators. 2.2 The second law of thermodynamics. 2.3 Carnot cycles and Carnot engines. 2.4* The thermodynamic temperature scale. 2.5 Entropy and maximum entropy theorem. 2.6 Some examples involving entropy changes.
