Question

Which statement about spontaneous and nonspontaneous processes is correct? Spontaneous processes are favored by a decrease in H, but nonspontaneous reactions are favored by an increase in H. Spontaneous processes are favored by a decrease in S, but nonspontaneous reactions are favored by an increase in S. An increase in S favors both spontaneous and nonspontaneous processes. A decrease in H favors both spontaneous and nonspontaneous processes.

Answer 1

I believe your answer would be the first one

hope this helps

Answer 2

Answer: Spontaneous processes are favored by a decrease in H, but nonspontaneous reactions are favored by an increase in H.

Explanation:

$\Delta G=\Delta H-T\Delta S$

$\Delta G$ = gibbs free energy

$\Delta H$ = change in enthalpy

$\Delta S$ = change in entropy

For a reaction to be spontaneous, $\Delta G$= -ve. For this $\Delta H$  has to be negative i.e. there should be a decrease in enthalpy and $\Delta S$ has to be positive i.e. there should be a increase in entropy.

$\Delta G=(-ve)-T(+ve)=-ve-ve=-ve$