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 is (ln2=0.7 )

One mole of an ideal gas is subjected to adiabatic expansion form initail state of (10"atm",300K) to final pressure of 1 atm against constant external pressure. Which of the following option contain correct change in thermodynamic parameters for the above process. (Given: gamma=(4)/(3))

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 -

One mole of monoatomic ideal gas at T(K) is exapanded from 1L to 2L adiabatically under constant external pressure of 1 atm . The final tempreture of gas in kelvin is

1 mole of monoatomic ideal gas subjected to irreversible adiabatic expansion against constant external pressure of 1 atm starting from initial pressure of 5 atm and initial temperature of 300K till the final pressure is 2 atm. What is the final temperature (in K) in the process? (take R = 2 cal/mol K).

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)]