What is the relationship between heat capacity at constant volume (Cv) and heat capacity at constant pressure (Cp) for an ideal gas?
Correct Answer: Cp = Cv + R
- Step 1: Understand what heat capacity means. Heat capacity is the amount of heat needed to change the temperature of a substance.
- Step 2: Know that there are two types of heat capacity: at constant volume (Cv) and at constant pressure (Cp).
- Step 3: Recognize that for an ideal gas, the heat capacity at constant pressure (Cp) is always greater than the heat capacity at constant volume (Cv).
- Step 4: Learn the formula that relates Cp and Cv for an ideal gas: Cp = Cv + R.
- Step 5: Identify R as the universal gas constant, which is a specific value (approximately 8.314 J/(mol·K)).
- Step 6: Conclude that the difference between Cp and Cv is equal to the universal gas constant (R).
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