Why does a diatomic gas have a greater energy content per mole than a monatomic gas at the same temperature?

Why does a diatomic gas have a greater energy content per mole than a monatomic gas at the same temperature?

A diatomic gas has more thermal energy than a monatomic gas at the same temperature because the molecules have rotational as well as translational kinetic energy. Isobaric requires MORE HEAT than Isochoric for the same change in Temperature!!!! This applies to all ideal gases, not just monatomic ones!

What is CV for monatomic gas?

The molar specific heat capacity of a gas at constant volume (Cv) is the amount of heat required to raise the temperature of 1 mol of the gas by 1 C at the constant volume. Its value for monatomic ideal gas is 3R/2 and the value for diatomic ideal gas is 5R/2.

What is molar specific heat capacity at constant pressure?

Then the molar heat capacity (at constant volume) would be cV,m = 1/2fR. where R is the ideal gas constant. According to Mayer’s relation, the molar heat capacity at constant pressure would be cP,m = cV,m + R = 1/2fR + R = 1/2(f + 2)R.

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How do you find heat capacity at constant pressure?

The specific heat at constant pressure for an ideal gas is given as (∂H∂T)V=cp=cv+R ( ∂ H ∂ T ) V = c p = c v + R .

Can a process be both isothermal and adiabatic?

Yes, an isothermal process can be adiabatic.

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