At temperature above 85 K, decarboxylation of acetic becomes a spontaneous process under standard state conditions. What is the standard entropy change (in J/K-mol) of the reaction.
`CH_(3)COOH (aq) rarr CH_(4)(g)+CO_(2)(g)`
`{:("Given :",DeltaH_(f)^(@)[CH_(3)COOH (aq)],=-484" kJ/mole"),(,DeltaH_(f)^(@)[CO_(2)(g)],=-392" kJ/mole"),(,DeltaH_(f)^(@) [CH_(4)(g)],=-75" kJ/mole"):}`

Explanation

At `85 K` the process must be at equilibrium under standard state condition:
`DeltaG^(@)=0`
`DeltaH^(@)=TDeltaS^(@)" "rArr" "DeltaS^(@)=(DeltaH^(@))/(T)=([-392-75-(-484)]xx10^(3))/(85)=2.00xx10^(2) J//K`-mol