Maximum work can a gas do if it is allowed to expand isothermally against
(A) Vacuum
(B) high pressure of surrounding
(C) Iow pressure of surrounding
(D) atmospheric pressure

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.

An ideal gas at 300K is expanded isothermally to double its volume,then pressure of the gas will be

70 gms of nitrogen gas was at 50 atm and 25^(@) C. (a) It was allowed to expand isothermally against a constant external pressure of one atmopshere. Calculate Deltau.Deltaq and Deltaw assuming that gas behaves ideally. (b) Also find out the maximum work that would be obtained if the gas expanded reversibly and isothermally to one atmosphere.

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]

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.

One mole of an ideal gas is heated at constant pressure from 0^(@)C to 100^(@)C . a. Calculate the work done. b. If the gas were expanded isothermally and reversibly at 0^(@)C from 1 atm to some othe pressure P , what must be the final pressure if the maixmum work is equal to the work in (a) ?

According to Langmuir adsorption isotherm, the amount of gas adsorbed at very high pressure:

What will be the work done when one mole of a gas expands isothermally from 15 L to 50 L against a constant pressure of 1 atm at 25^(@)C ?

5 mole of an ideal gas expand isothermally and irreversibly from a pressure of 10 atm to 1 atm against a constant external pressure of 2 atm. w_(irr) at 300 K is :

When two moles of hydrogen expands isothermally against a constant pressure of 1 atm , at 25^@C from 15 L to 50 L , the work done (in litre atm) will be