How much energy is evolved during the formation of 197 g of fe, according to the reaction below? fe2o3 (s) + al (s) → al2o3 (s) + fe (s) δh°rxn = - 852 kj?

Question

Kyler Dorsey

Chemistry

7 December, 06:58

How much energy is evolved during the formation of 197 g of fe, according to the reaction below? fe2o3 (s) + al (s) → al2o3 (s) + fe (s) δh°rxn = - 852 kj?

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Answers (1)

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Jamar Woodard · Answer 1

Answer is: 1,51·10³ kJ is evolved during the formation.

Chemical reaction: Fe₂O₃ (s) + Al (s) → Al₂O₃ (s) + Fe (s); ΔH°rxn = - 852 kJ.

m (Fe) = 197 g.

n (Fe) = m (Fe) : M (Fe).

n (Fe) = 197 g : 55,85 g/mol.

n (Fe) = 3,527 mol.

Use proportion: 2 mol (Fe) : - 854 kJ = 3,527 mol (Fe) : ΔH°rxn.

ΔH°rxn = - 854 kJ · 3,527 mol : 2 mol.

ΔH°rxn = - 1510 kJ = - 1,51·10³ kJ.