Match the following processes with their corresponding entropy changes:

$a$. Liquid to vapor conversion	$1$. $\Delta S = 0$
$b$. Reaction not spontaneous at any temperature,$\Delta H = (+)$	$2$. $\Delta S = (+)$
$c$. Reversible expansion of an ideal gas	$3$. $\Delta S = (-)$

(A) The correct matches are:
$a-2$: Conversion of liquid to vapor increases disorder,so $\Delta S = (+)$.
$b-3$: For a reaction to be non-spontaneous at all temperatures where $\Delta H = (+)$,the entropy change $\Delta S$ must be negative $((-))$ because $\Delta G = \Delta H - T\Delta S$. If $\Delta S = (-)$,then $\Delta G$ will always be positive.
$c-1$: For a reversible process,the entropy change of the system and surroundings is zero,but specifically for the reversible expansion of an ideal gas in an isolated system,$\Delta S = 0$ is often considered in specific contexts,though generally,it refers to the equilibrium state.
Correct sequence: $a-2, b-3, c-1$.