The entropy change involved in the isothermal reversible expansion of 2 moles of an ideal gas from a volume of `10 dm^(3)` to a volume of `100dm^(3)` at `27^(@)C` is

Options

A. `35.8 " J mol"^(-1) K^(-1)`
B. `32.3 "J mol"^(-1) K^(-1)`
C. `42.3 "J mol"^(-1) K^(-1)`
D. `38.3 "J mol"^(-1) K^(-1)`

Answer

D

Explanation

For isothermal reversible expansion
`Delta S = nR ln (V_2)/(V_1) =2 xx 8.314 xx 2.303 log (100)/(10)`
`= 38.3 J " mol " ^(-1) K^(-1)`