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

Answer

C

Explanation

For isothermal reversible expansion of an ideal gas, `DeltaS = nR ln. (V_(2))/(V_(1))=2 xx 8.314 xx 2.303 log. ( 100)/(10)`
`= 38.3 J mol^(-1) K^(-1)`