Use the ΔH°f information provided to calculate ΔH°rxn for the following:

ΔH°f (kJ/mol) SO2Cl2 (g) + 2 H2O(l) → 2 HCl(g) + H2SO4(l) ΔH°rxn = ?
SO2Cl2(g) -364
H2O(l) -286
HCl(g) -92
H2SO4(l) -814

Thanks for any help!

It isn't difficult to come to this conclusion (basically, the total enthalpy gain or loss results from the consumption [-] of reactants and formation [+] of products):
ΔH°r = - ΔH°f (reactants) + ΔH°f (products)

And according to the reaction:
SO2Cl2 + 2 H2O → 2 HCl + H2SO4
ΔH°r = - (ΔH°f SO2Cl2 + 2*ΔH°f H2O ) + (2*ΔH°f HCl + ΔH°f H2SO4)

Now just replace each ΔH°f by it's value. Sorry, I'm too lazy to do that.