Explain why for an ideal gas there is a difference between the molar specific he
ID: 2207467 • Letter: E
Question
Explain why for an ideal gas there is a difference between the molar specific heat at a constant volume and the molar specific heat at constant pressure.Explain how the number of degrees of freedom that a gas molecule has for storing energy contributes to the molar specific heat of the gas.
Explain why and how an object at a higher temperature transfers heat to an object of lower temperature and not the other way around.
Describe the four postulates of kinetic theory and explain its central conclusions.
Explanation / Answer
Specific heat of a gas is numerically equal to the amount of heat necessary to raise the temperature of unit mass of gas by 1°C. In order to raise the temperature of unit mass of a gas through 1°C more heat will be required if the gas was kept at constant pressure than when it is at constant volume. (i) Molar Specific heat capacity at constant Volume: The amount of heat required to raise the temperature of 1 mole of gas by 1 °C at constant volume is called the molar specific heat and it is represented by Cv. Cv = (?Q/m?t)v = constant By first law of thermodynamics ?Q = ?U + W But W = 0 for isochoric process, then ?Q = ?U by definition of specific heat ?Q = nCv?T
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