This question was asked in the JEE examination of 2017 :
[A] option is incorrect since the system is losing heat and hence $ \Delta S\lt0$
[B] Lets assume we have an endothermic reaction $\ce { A <=> B - Heat} $
Now if we increase the temperature, the reaction will shift to the product side and hence the entropy of the surroundings will decrease more as compared to the initial conditions. Therefore the Unfavourable change in entropy(decrease in entropy) should increase.
[C] Though the reaction is endothermic, since we are supplying heat to the system, the net change in entropy of the system is positive.
[D] Lets assume another exothermic reaction $ \ce{A<=>B + Heat}$.
When we increase the temperature, the reaction will shift to the left side and hence less heat will be given off to the surroundings. Therefore, favourable change in entropy(increase in entropy) decreases.
Hence, according to me, the correct answer should only be [D], but [B] option is also given correct. What is the error in my explanation?
