Answer:
B. ∆H<0
Step-by-step explanation:
The change in enthalpy (∆H) for a reaction is a measure of the amount of heat that is absorbed or released during the reaction. A positive ∆H indicates that the reaction is endothermic, meaning that heat is absorbed during the reaction. A negative ∆H indicates that the reaction is exothermic, meaning that heat is released during the reaction. A ∆H of zero indicates that the reaction is thermally neutral, meaning that there is no heat transfer during the reaction.
In the given reaction, C2H6 (l) → C2H6 (s), the substance changes from a liquid to a solid, which typically involves a decrease in entropy (or disorder) of the system. This means that the reaction is exothermic, because the decrease in entropy is usually accompanied by a release of heat. Therefore, we would expect the ∆H for this reaction to be negative, which means that B. ∆H<0 is likely to be true for this reaction.