What is the relationship between heat capacity at constant pressure (Cp) and heat capacity at constant volume (Cv)?

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Q: What is the relationship between heat capacity at constant pressure (Cp) and heat capacity at constant volume (Cv)?

Solution: For an ideal gas, Cp is always greater than Cv because it includes the work done against the atmospheric pressure.

Steps: 6

Step 1: Understand what heat capacity means. Heat capacity is the amount of heat needed to change the temperature of a substance.
Step 2: Learn about constant pressure (Cp). Cp is the heat capacity when the pressure of the gas does not change.
Step 3: Learn about constant volume (Cv). Cv is the heat capacity when the volume of the gas does not change.
Step 4: Recognize that when a gas is heated at constant pressure, it can expand. This expansion does work against the surrounding pressure.
Step 5: Understand that this work done requires extra energy, which is why Cp is greater than Cv.
Step 6: For an ideal gas, the relationship can be summarized as Cp = Cv + R, where R is the gas constant.