Answer:
The answer to your question is: ΔH = -849.5 KJ/mol
Explanation:
Data
ΔH = ?
H Fe2O3 = -825.5 KJ/mol
H Al2O3 = -1675 KJ/mol
H Al = 0 KJ/mol
H Fe = 0 KJ/ mol
Reaction
2Al(s) + Fe2O3(s) → 2Fe(s) + Al2O3(s)
ΔH = H products - H reactants
ΔH = H Al2O3 - H Fe2O3
ΔH = -1675 - (- 825.5)
ΔH = -1675 + 825.5
ΔH = -849.5 KJ/mol
Answer - A, B, D, E
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