Enthalpy formation from enthalpy reaction

Question

A scientist measures the standard enthalpy change for the following reaction to be 6.6 kJ :

Fe(s) + 2 HCl(aq)FeCl₂(s) + H₂(g)

Based on this value and the standard enthalpies of formation for the other substances, the standard enthalpy of formation of HCl(aq) is   kJ/mol.

standard enthalpy

HCl= −92.3 kJ/mol

2 HCl(aq)=−92.3 kJ/mol

FeCl₂(s)= −341.79kJ/mol

Answer 1

Fe(s) + 2 HCl(aq) ==> FeCl₂(s) + H₂(g)

∆H_rxn = ∑∆Hf_products - ∑Hf_reactants

6.6 kJ = (-341.79 + 0) - (0 + 2x)

6.6 = -341.79 - 2x

2x = -348.39

x = -174.2 kJ / mol HCl

** The question asks for ∆Hf for HCl but then it gives the ∆Hf for HCl as -92.3 kJ/mole. Was that supposed to be an option or was that the actual value? Not sure exactly what is given and what is asked for in this question.