Question

how do heat capacity at constant pressure are related.

Answer 1

For an ideal gas at constant pressure, it takes more heat to achieve the same temperature change than it does at constant volume. At constant volume all the heat added goes into raising the temperature. At constant pressure some of the heat goes to doing work.

Q = nCPΔT

For an ideal gas, applying the First Law of Thermodynamics tells us that heat is also equal to:

Q = ΔEint + W

At constant pressure W = PΔV = nRΔT

For a monatomic ideal gas, where ΔEint = (3/2)nRΔT, we get:

Q = (3/2)nRΔT + nRΔT = (5/2)nRΔT

So, for a monatomic ideal gas:

CP = (5/2)R

For diatomic and polyatomic ideal gases we get:

diaatomic: CP = (7/2)R

polyatomic: CP = 4R

Answer 2

hello friend
Heat capacity at constant pressure
For an ideal gas at constant pressure,it makes more heat to achieve the same temperature change than it does at constant volume. At constant volume all the heat added goes into raising the temperature
hope it helped you
plz mark me as brianliest