The pressure-volume of varies thermodynamic process is shown in graphs:

Work is the mole of transference of energy. It has been observed that reversible work done by the system is the maximum obtainable work.
`w_(rev) gt w_(irr)`
The works of isothermal and adiabatic processes are different from each other.
`w_("isothermal reversible") = 2.303 nRT log_(10) ((V_(2))/(V_(1)))`
`= 2.303 nRT log_(10)((P_(2))/(P_(1)))`
`w_("adiabatic reversible") = C_(V) (T_(1)-T_(2))`
The `q` value and work done in isothermal reversible expansion of one mole of an ideal gas from initial pressure of `1` bar to final pressure of `0.1` bar at constant temperature `273K` are:

Options

A. `5.22 kJ, -5.22 kJ`
B. `+6.22 kJ, 6.22 kJ`
C. `5.22 J, 5.22 J`
D. `-6.22 J, -6.22 J`

Explanation

`w =- 2.303 nRT log((P_(1))/(P_(2)))`
`=- 2.303 xx 1xx 8.314 xx 273 log ((1)/(0.1)) =- 5.227 kJ`
`q = -w =+ 5.227 kJ` for isothermal process