`1` mole of an ideal diatomic gas undergoes a reversible polytropic process `(PV^(2)="constant")`. The gas expand from initial volume of `1` litre and temp `300 K` to final volume `3` lit. Claculate change in internal energy (approx).

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))]

2 moles of an ideal monoatomic gas undergo a reversible process for which PV^(2)= constant. The gas sample is made to expand from initial volume of 1 litre of final volume of 3 litre starting from initial temperature of 300 K. find the value of DeltaS_("sys") for the above process. Report your answer as Y where DeltaS_("sys")=-YRIn3

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

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 :

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 :

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 :

In the polytropic process PV^2 = constant, is the gas cooled'or heated with increase in volume.

A gas of volume changes 2 litre to 10 litre at constant temperature 300K, then the change in internal energy will be :