1mole of a triatomic non-linear ideal gas is subjected to an adiabatic process from initial temperature 400K and pressure 32 atm to final pressure 2 atm.If the expansion is carried out against vacuum the entropy change (in cal `K^(-1)`) for the system ln2 = 0.7

In an isothermal process at 300 K, 1 mole of an ideal gas expands from a pressure 100 atm against an external pressure of 50 atm. Then total entropy change ("Cal K"^(-1)) in the process is -

The temperature of 5 moles of a gas is decreased by 2K at constant pressure of 1 atm. Indicate the correct statement

One mole of an ideal monoatomic gas at 27^(@)C is subjected to a reversible isoentropic compression until the temperature reached to 327^(@)C . If the initial pressure was 1.0 atm , then find the value of ln P_(2) ( Given : ln 2=0.7)

1 mole of an ideal gas is expanded from an initial pressure of 1 bar to final pressure of 0.1 bar at constant temperature of 273 K. Predict which of the following is not true?

One mole of an ideal monoatomic gas expands isothermally against constant external pressure of 1 atm from initial volume of 1l to a state where its final pressure becomes equal to external pressure. If initial temperature of gas is 300K then total entropy change of system in the above process is: [R =0.082L atm mol^(-1)K^(-1)= 8.3J mol^(-1) K^(-1) ]

One mole of an ideal monoatomic gas expands isothermally against constant external pressure of 1 atm from intial volume of 1L to a state where its final pressure becomes equal to external pressure. If initial temperature of gas in 300 K then total entropy change of system in the above process is: [R=0.0082L atm mol^(-1)K^(-1)=8.3J mol^(-1)K^(-1)]

1mol of an ideal gas at 400K and 10atm is allowed to expand, adiabatically, against 2.0atm external pressure. Find the final temperature of the gas. [Use: C_(v) = (5)/(2)R]

One mole of an ideal gas (C_(v,m)=(5)/(2)R) at 300 K and 5 atm is expanded adiabatically to a final pressure of 2 atm against a constant pressure of 2 atm. Final temperature of the gas is :

A sample of certain mas s of an ideal polyatomic gas is expanded against constant pressure of 1 atm adiabatically from volume 2L , pressure 6 atm and temperature 300K to state where its final volume is 8L . Then calculate entropy change (in J/k) in the process.(Neglect vibrational degress of freedom)[1 L atm = 100 J ,log 2 =0.3 , log 3 = 0.48 , log e = 2.3] (approximate integer)

When 1mol of a monoatomic ideal gas at TK undergoes adiabatic change under a constant external pressure of 1atm , changes volume from 1 L to 2L . The final temperature (in K) would be