Q = nCVΔT
For an ideal gas, applying the First Law of Thermodynamics tells us that heat is also equal to:
Q = ΔEint + W, although W = 0 at constant volume.
For a monatomic ideal gas ΔEint = (3/2)nRΔT
Comparing our two equations
Q = nCVΔT and Q = (3/2)nRΔT
we see that, for a monatomic ideal gas:
CV = (3/2)R
For diatomic and polyatomic ideal gases we get:
diatomic: CV = (5/2)R
polyatomic: CV = 3R
This is from the extra 2 or 3 contributions to the internal energy from rotations.