One mole of an ideal gas at STP is heated to `27^@C` and compressed to 1.5 atm. Calculate `triangleE` and `triangleH` for the change in state. Assume `C_v = 3/2 R` for the ideal gas.

One mole of an ideal monoatomic gas is heated at constant pressure from 0^@C to 100^@C . Calculate work done.

One mole of an ideal monatomic gas is heated at a constant pressure from 0^(@)C to 100^(@)C . Then the change in the internal energy of the gas is (given R = 8.32 J cdot mol cdot k^(-1))

In case of 1 mol of an ideal gas, write down the value of C_(v) - C_(p) .

At 27^(@)C, 4.2 g N_(2) gas is expanded reversibly and isothermally from a pressure of 10 atm to 1 atm. Calculate q, Delta U, Delta H and w for this expansion. Assume N_(2) gas behaves ideally.

A 5 mol sample of an ideal gas is compressed isothermally and irreversible from 1.5 atm to 15 atm at 27^(@)C . Calculate the work done on the gas in calorie unit.

The pressure of 3 mol of an ideal gas is 10 atm at 27^(@)C . Calculate work done by the gas when it is expanded isothermally against an external pressure of 1 atm.

One mole of carbon-dioxide was found to occupy a volume of 1.32 litre at 48^(@) C and at a pressure of 16.4 atm. Calculate the pressure of the gas that would have been expected to behave ideally and non-ideally.

70 cals of heat is required to raise the temperature of 2 moles of an ideal gas at constant pressure from 30^@C to 35^@C . Calculate the amount of heat required to raise the temperature of same gas through same range at constant volume. (R = 2 cal / mole ^@C )