Hi! We did an experiment where we should determent ΔH of Mg per mol. Mg(s) + 2HCI (aq) → MgCl2 (aq)+ H2 (g)

1. qHCl=CmΔT.
MHCl=26,56 gram
ΔT= 31,1 C
CH2O= 4,2 J/ (g · K)
qHCl=4,2 J/ (g · K) x 26,56gram x 31,1 C
qHCl= 3469,2672 J/mol

MMg= 24,3 gram/mol
mMg= 0,36 gram
nMg= mMg/Mmg
nmg= 0,36 gram/ 24,3 gram/mol
nmg= 0,0148148148 mol

nmg= 0,0148148148 mol
qHCl=3469,2672 J/mol
ΔH= 3469,2672 J/mol/ 0,0148148148 mol
ΔHHCl= 234175,5362 J/mol
ΔHMg= - ΔHHCl
ΔHMg= - 234175,5362 J/mol

This is my calculations how ever I want to compare it to the real value by using this equation. Have I made it right? I want to know the ΔHMg.

∆Hº(reaktion) = ∆Hºn(produkter) - ∆Hºn(reaktanter)

Produkter
Mg= -462.0 kj
Cl= -167.2
MgCl2 (aq)= -462.0 + (-167.2 x 2) = -796.6 kJ/mol

Reaktanter
HCl (aq) = -167.4 kJ/mol
2HCl= -167.4 kJ/mol x 2 = 334,8

∆Hº(reaktion) = (-796.8 kJ/mol + 0) - (0 + -167.4 kJ/mol x 2)
∆Hº(reaktion) = -462 kJ/mol

Is it the ∆H for the whole reaktions per mol or is it for mg? I get so confused!