Final answer:
To calculate the enthalpy change for creating 2 moles of liquid sulfuric acid, one needs to consult the standard enthalpies of formation for all reactants and products, then apply Hess's law to find the total ΔH for the reaction.
Step-by-step explanation:
The question involves calculating the enthalpy change for the reaction where gaseous SO2Cl2 reacts with liquid water to form hydrogen chloride gas and liquid sulfuric acid. To find this value, one would typically look up the standard enthalpies of formation for each of the reactants and products from Appendix G or a similar reference. The enthalpy change (ΔH) for the reaction is then calculated using Hess's law: the sum of the standard enthalpies of formation of the products minus the sum of the standard enthalpies of formation of the reactants.
Since the question asks specifically about the formation of 2 moles of sulfuric acid, the standard enthalpy of formation of liquid sulfuric acid would be multiplied by 2, and the values for the other reactants and products would be accounted for according to their stoichiometric ratios in the balanced chemical equation.