Question

The specific heat of an ideal gas at constant pressure (CP) is always larger than its specific heat at constant volume (CV): CP = CV + R where R is the ideal gas constant: R = 8.31 Joules/(mole-K). Explain clearly in your own words why CP > CV always, using (among other things) the first law of thermodynamics.

          The specific heat of an ideal gas at constant pressure (CP) is always larger than its specific heat at constant volume (CV):

CP = CV + R

where R is the ideal gas constant: R = 8.31 Joules/(mole-K). Explain clearly in your own words why CP > CV always, using (among other things) the first law of thermodynamics.

The specific heat of an ideal gas at constant pressure (CP) is always larger than its specific heat at constant volume (CV):

CP = CV + R

where R is the ideal gas constant: R = 8.31 Joules/(mole-K). Explain clearly in your own words why CP > CV always, using (among other things) the first law of thermodynamics.

Added by Kirk O.

University Physics with Modern Physics

Hugh D. Young 14th Edition

Instant Answer

Solved by Expert Shaiju T

04/28/2022

Step 1

** Show more…

Show all steps

Thanks for your feedback!

The specific heat of an ideal gas at constant pressure (Cp) is always larger than its specific heat at constant volume (Cv): Cp = Cv + R where R is the ideal gas constant: R = 8.31 Joules/(mole-K). Explain clearly in your own words why Cp is always larger than Cv, using (among other things) the first law of thermodynamics.