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

Answer

a

Explanation

Entropy change for an isothermal process is
`DeltaS=2.303R log((V_(2))/(V_(1)))`
`DeltaS=2.303xx2xx8.314xxlog(100/10)`
`=38.294 J mol^(-1) K^(-1)`