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

Answer

A

Explanation

`DeltaS=nRln.(V_(2))/(V_(1))=2.303 nR log. (V_(2))/(V_(1))`
`2.303xx2xx8.314xxlog.(100)/(10)`
`=38.3 J mol^(-1) K^(-1)`.