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?

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.

Answer : The energy evolved in the reaction is 1499.52 kJ

Explanation :  Given,

Mass of Fe = 197 g

Molar mass of Fe = 56 g/mole

Enthalpy of reaction = -852 kJ

First we have to calculate the moles of Fe.

Now we have to calculate the energy evolved in the reaction.

From the balanced chemical reaction we conclude that,

As, 2 mole of Fe evolved energy = 852 kJ

So, 3.52 mole of Fe evolved energy =

                                                         = 1499.52 kJ

Therefore, the energy evolved in the reaction is 1499.52 kJ

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