Calculate work done by `1` mole of ideal gas expand isothermally and irreversibly from pressure of `5` atm to `2` atm against a constant external pressure of `1` atm at `300 K` temperature.

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 1 atm. w_(irr) at 300 K is :

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 1 atm. w_(irr) at 300 K is :

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 :

5 mole of an ideal gas expands isothermally and irreversibly from a pressure of 10 atm to 1 atm against a contant external pressure of 1 atm. W_("irr") at 300K is:

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 1 atm. w_(irr) at 300 K is : (a) -15.921 kJ (b) -11.224 kJ (c) -110.83 kJ (d)None of these

Calculate the work done by 1.0 mol of an ideal gas when it expands at external pressure 2atm from 10atm to 2atm at 27^(@)C