2 moles of an ideal mono atomic gas undergoes reversible expansion from (4L,[400K) to 8L such that `TV^(2)= constant` The change in enthalpy of the gas is

Five moles of an ideal gas undergoes reversible expansion from 1 L to 4 L at 27°C. The work done and enthalpy change for the process respectively are

2 mole of an ideal monoatomic gas undergoes a reversible process for which PV^(2)=C . The gas is expanded from initial volume of 1 L to final volume of 3 L starting from initial temperature of 300 K. Find DeltaH for the process :

1 mole of an ideal gas undergoes an isothermal reversible expansion form 10 atm to 1 atm at 300 K. What will be the work done ?

A perfect gas undergoes a reversible adiabatic expansion from (300 K, 200 atm) to (90 K, 10 atm). Find the atomicity of gas.

A defintie amount of diatomic ideal gas undergoes reversible adiabatic expansion from 10 L, 127^(@)C to 'V'L,-73^(@)C. The molar heat capacity of gas at constant volume is : [Given : R=8.3JK^(-1),ln 2 =0.7.ln 30=3.4]

Three moles of an ideal gas expands reversibly under isothermal condition form 2 L to 20 L at 300 K. The amount of heat-change (in kJ/mol) in the process is -

1 mole of an ideal diatomic gas undergoes a reversible polytropic process (PV^(2)=K) .The gas expands from initial volume of 1L to 3L and initial temperature of 300K what is the change in internal energy |Delta U| in cal [(R=2calmol^(-1)K^(-1))]

One mole of an ideal gas undergoes change of state from (4 L, 3 atm) to (6 L, 5 atm). If the change in internal energy is 45 L-atm then the change of enthalpy for the process is