Two liters of `N_(2)` at `0^(@)C` and `5` atm pressure is expanded isothermally against a constant external pressure of `1` atm untill the pressure of gas reaches `1` atm. Assuming gas to be ideal, claculate the work of expansion.

Two liters of nitrogen gas at 0^(@)C and "5" atm pressure expanded isothermally against a constant external pressure of "1" atm until the pressure of gas reaches "1" atm.Assuming the gas to be ideal,find the magnitude of work of expansion in lit atm

2.8 g of N_(2) gas at 300 K and 20 atm was allowed to expand isothermally against a constant external pressure of 1 atm. Calculate W for the gas.

28g of N_(2) gas at 300 K and 20 atm was allowed to expand isothermally against a constant external pressure of 1 atm , q for the gas is (R=0.082) .

Consider the same expansion, but this time against a constant external pressure of 1 atm.

2.8g of N_(2) gas at 300K and 20atm was allowed to expand isothermally against a constant external pressure of 1atm . Calculate DeltaU, q, and W for the gas.

10 litre of an ideal gas at 25 atm and 27^(@)C is expanded isothermally to 1 atm against a constant external pressure of 760 torr. Calualate work done by the gas in litre-atm:

A gas expands from 4.0 L to 4.5 L against a constant external pressure of 1 atm. The work done by the gas is (1 L-atm = 101.3 J)

A gas expands by 0.372 litre against a constant pressure of 1atm . Find the work done in cal.

A gas expands from 10 litres to 20 litres against a constant external pressure of 10 atm. The pressure-volume work done by the system is

A gas expands by 0.5L against a constant pressure of 1 atm . Calculate the work done in joule and calorie.