If `1.0` kcal of heat is added to `1.2 L` of `O_(2)` in a cyclinder at constant pressure of `1` atm, the volume increases to `1.5L`. Calculate `Delta U` and `Delta H` of the process. `(1L-atm=100J)`

If 1.0 kcal of heat is added to 1.2 L of O_(2) in a cyclinder of constant pressure of 1 atm , the volume increase to 1.5 L . Calculate DeltaU and DeltaH of the process.

Calculate the internal energy change for the process in which 1.0 kcal of heat is added to1 .2 litre of O_(2) gas in a cyclinder at constant pressure of 1.0 atm and the volume changes to 1.5 litre.

The temperature of 1 mol of an ideal monoatomic gas at constant pressure of 1 atm changes from 25^(@)C and 50^(@)C . Calculate Delta U and Delta H in this process, (C_(V)=(3)/(2)R) .

A gas expands from 1l to 6l against a constant pressure of 1 atm and it absorbs 500J of heat Delta U is

One mole of an ideal gas is expanded from a volume of 3L to 5L under a constant pressure of 1 atm. Calculate the work done by the gas.

When 1 mole of an ideal gas at 20 atm pressure and 15 L volume expands such that the final pressure becomes 10 atm and the final volume becomes 60 L. Calculate entropy change for the process (C_(p.m)=30.96 J "mole"^(-1) K^(-1))

A gas confined in a cylinder with a frictionless piston is made to expand from 1L to 5L under constant pressure of 1.5 atm. During the process, 800J of heat is supplied from external source. Calculate the change in internal energy off the gas. (1L*atm=101.3J) .

A gas expands from 4.0 L to 4.5 L against a constant external pressure of 1 atm. The work done by the gas is (1 L-atm = 101.3 J)

A gas expands from 4.0 L to 4.5 L against a constant external pressure of 1 atm. The work done by the gas is (1 L-atm = 101.3 J)