Which one of the following is correct for a spontaneous reaction at any temperature ?

A spontaneous reaction is a reaction that favors the formation of products at the conditions under which the reaction is occurring.

$\Delta H<0$ and $\Delta S>0$

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

For the reaction to be spontaneous, $\Delta G$ should be negative, this works if $\Delta H$ is negative and $\Delta S$ is positive.

Hence the correct answer is (B) $\Delta \mathrm{H}=-\mathrm{ve},\Delta \mathrm{S}=-\mathrm{ve},\Delta \mathrm{G}=-\mathrm{ve}$.