Final answer:
The standard enthalpy change (ΔH°) for the reaction in question cannot be calculated directly from the provided reactions due to the inclusion of unrelated species, and the lack of entropy values prevents the calculation of ΔSsys. Instead, tabulated standard enthalpy and entropy values should be used if available.
Step-by-step explanation:
To calculate the standard enthalpy change (ΔH°) for the reaction 2Al(s) + 3Cl2(g) → 2AlCl3(s), we need to use Hess's Law and combine the enthalpy changes of known reactions to derive the enthalpy change for the target reaction. Unfortunately, the reactions listed in the question (ii to v) do not directly relate to the reaction in question as they include species like HCl that are not involved in the target reaction. Therefore, a direct calculation using the given reactions is not possible; instead, the enthalpy of formation or tabulated standard enthalpy values for reaction (i) should be used if available.
The formula to calculate enthalpy changes using Hess's Law is ΔH° = ∑ΔH°(products) - ∑ΔH°(reactants). In this example, since we do not have individual reaction enthalpies, we cannot calculate ΔH° for the reaction directly from the given reactions.
Note: The student's original question appears to ask for the calculation of ΔSsys, but without the standard entropy values for the reactants and products, we cannot calculate this either, and it appears to be a typo or an error in the original question.