Calculate total entropy change for the transition of 1 mole of solid sulphur from its monoclinic form to the rhombic form at 400 K, id `DeltaH=-400J//"mole"` for this transition and assume the surrounding to be in a bath of water at `27^(@)C`

Options

A. `-1J//k`
B. `+0.33J//k`
C. `1.67J//k`
D. `0.66J//k`

Answer

B

Explanation

`DeltaS_(sys)=-(400)/(400)=-1J//k`
`DeltaS_("surr")=+(400)/(300)=(4)/(3)J//k`
`DeltaS_(T)=-1+(4)/(3)=+(1)/(3)J//k`