Under constant-volume conditions, 3700 J of heat is added to 2.2 moles of an ideal gas. As a result, the temperature of the gas increases by 81.0 K. How much heat would be required to cause the same temperature change under constant-pressure conditions? Do not assume anything about whether the gas is monatomic, diatomic, etc.

Under constant-volume conditions, 3700 J of heat is added to 2.2 moles of an ideal gas. As a result, the temperature of the gas increases by 81.0 K. How much heat would be required to cause the same temperature change under constant-pressure conditions? Do not assume anything about whether the gas is monatomic, diatomic, etc.