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. `38.3JK^(-1)`
B. `35.8JK^(-1)`
C. `32.3JK^(-1)`
D. `42.3JK^(-1)`

Answer

A

Explanation

Entropy change for `n` moles of isothenal expansion of an ideal gas from volume `V_(1)` to volume `V_(2)` is
`DeltaS=2.303nR"log"(V_(2))/(V_(1))` ltbr. Hence, `n=2` , `V_(2)=100dm^(3) , V_(1)=10dm^(3)`
`2.303xx2xx8.3143"log"(100)/(10)`
`=38.296Jmol^(-1)K^(-1)`