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Molar heat capacity is greater at constant pressure than at constant volume because at constant P, some of the heat goes into expansion work which means there will be less energy left over to raise the temperature unlike at constant V, where no expansion work is done so all the energy goes into raising the temperature.
To expand on the previous two replies, the book gave the example of argon which has a constant volume heat capaccitg of 12.8, so when using the equation, you get 12.8 + 8.3= 21.1 for the constant pressure value. That is 65% greater than the constant volume value.
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