Answer:
Option A and B
Explanation:
(a) DeltaH = -84 kj mol-2 (-20 kcal mol-1), DeltaS = +125j mol-2K-1)(+30 cal mol-1 K-1)
Delta G = Delta H – T * DS
Substituting the given values, we get –
Delta G = -84 -298 *(125/1000) = -121.25 KJ/mol
Delta G is negative hence the process is spontaneous and will not violate the second law of thermodynamics
(b) DeltaH = -84 kj mol-2 (-20 kcal mol-1), DeltaS = -125j mol-2K-1)(-30 cal mol-1 K-1)
Delta G =-84 -298 *(-125/1000) = -46.75 KJ/mol
Delta G is negative hence the process is spontaneous and will not violate the second law of thermodynamics
(c) DeltaH = +84 kj mol-2 (+20 kcal mol-1), DeltaS = +125j mol-2K-1)(+30 cal mol-1 K-1)
Delta G = 84 -298 *(125/1000) = +46.75 KJ/mol
Delta G is positive hence the process is non-spontaneous and will violate the second law of thermodynamics
(d) DeltaH = +84 kj mol-2 (+20 kcal mol-1), DeltaS = +125j mol-2K-1)(-30 cal mol-1 K-1)
Delta G = 84 -298 *(-125/1000) = + 121.25 KJ/mol
Delta G is positive hence the process is non-spontaneous and will violate the second law of thermodynamics
