What is the relationship between heat capacity at constant pressure (Cp) and hea

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

Options:

Correct Answer: Cp > Cv

Solution:

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

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

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

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.

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