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

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).

For a monoatomic ideal gas undergoing an adiabatic change, the relation between temperature and volume TV^(x) = constant, where x is

For a monoatomic ideal gas undergoing an adiabatic change, the relation between temperature and volume TV^(x) = constant, where x is

One mole of an ideal monoatomic gas at temperature T and volume 1L expands to 2L against a constant external pressure of one atm under adiabatic conditions, then final temperature of gas will be:

One mole of an ideal monoatomic gas at temperature T and volume 1L expands to 2L against a constant external pressure of one atm under adiabatic conditions, then final temperature of gas will be:

One mole of an ideal monoatomic gas at temperature T and volume 1L expands to 2L against a constant external pressure of one atm under adiabatic conditions, then final temperature of gas will be: