Specific heat capacity of gases (Cp) is the amount of energy required to raise the temperature of a unit mass of a gas by 1 degree Celsius at constant press...
Specific heat capacity of gases (Cp) is the amount of energy required to raise the temperature of a unit mass of a gas by 1 degree Celsius at constant pressure. It is an extensive property, meaning it requires knowledge of the gas's specific heat capacity and the amount of gas present.
Specific heat capacity of gases (Cv) is the amount of energy required to raise the temperature of a unit mass of a gas by 1 degree Celsius at constant volume. It is a fundamental property, related to both Cp and the ideal gas law.
Key differences between Cp and Cv:
Cv is included in Cp: Cp is the total heat capacity, including both the work done by the gas during expansion and the energy transferred to its surroundings during compression.
Cv is used in the ideal gas law: The ideal gas law states that PV = nRT, where P is the pressure, V is the volume, n is the number of moles of gas, R is the ideal gas constant, and T is the temperature. Cp is a constant used in the ideal gas law, while Cv is a property of the gas.
Examples:
Cp of air at 1 atm and 25°C is approximately 1 calorie/(gram degree Celsius). This means that it takes 1 calorie of energy to raise the temperature of 1 gram of air by 1 degree Celsius at constant pressure.
Cv of hydrogen gas at 1 atm and 0°C is approximately 2 calories/(gram degree Celsius). This means that it takes 2 calories of energy to raise the temperature of 1 gram of hydrogen gas by 1 degree Celsius at constant volume.
Understanding specific heat capacity is crucial for comprehending the behavior of gases, as it provides valuable information about how energy is transferred and the changes in state that occur when gases expand or contract