Given the Following Thermochemical Equations: (KJ)

Given the following thermochemical equations: (kJ)
4 FeS₂(s) + 11O₂(g) → 2 Fe₂O₃(s) + 8 SO₂(g) ΔH° = -3307.9
2 H₂S(g) + 3O₂(g) → 2 H₂O(l) + 2 SO₂(g) - 1125.2
4 FeO(s) + O₂(g) → 2 Fe₂O₃(s) - 578.2
2 Fe(s) + O₂(g) → 2 FeO(s) - 544
H₂(g) + S(rh) → H₂S(g) - 20.2
2 H₂(g) + O₂(g) → 2 H₂O(l) - 571.7
Compute the ΔH°f for FeS₂(s) in kJ/mol.

A) -1233.9 kJ
B) -2893.9 kJ
C) -24.3 kJ
D) -183.5 kJ
E) -70.0 kJ