Chemistry problem?

Molar mass of Fe₂O₃ = 55.85×2 + 16.00×3 = 159.7 g/mol

Fe₂O₃(s) + 2Al (s) ⇌ 2Fe (s) + Al₂O₃(s) .... ∆H(rxn) = -8.5 × 10⁵ J
When 1 mole of Fe₂O₃ reacts, 8.5 × 10⁵ J of energy is released.
When 159.7 g of Fe₂O₃ reacts, 8.5 × 10⁵ J of energy is released.
Let m g be the mass of Fe₂O₃ reacted when 852 J of energy is released.

159.7/y = (8.5 × 10⁵)/852
y = 159.7 × [852/(8.5 × 10⁵)]
y = 0.16

Mass of Fe₂O₃ reacted = 0.16 g