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 const

1.	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)]
Answer» 0 R ln (24.6) R ln (2490) `(3)/(2)` R ln (24.6) Solution :`DELTA S = nR ln [(V_(2))/(V_(1))] = R "ln " (P_(1))/(P_(2))` `P_(1) = (1 XX R xx 300)/(1) = 24.6`