Problem: How much energy is evolved during the reaction of 51.2 g of Al, according to the reaction below?Assume that there is excess Fe2O3.Fe2O3(s) + 2 Al(s) → Al2O3(s) + 2 Fe(s)          ΔH°rxn = -852 kJ A) 51.2 kJ B) 448 kJ C) 224 kJ D) 1617 kJ E) 808 kJ

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FREE Expert Solution

Use the balanced equation and provided mass of Al to find the energy released 

Recall that the provided Δ°H will account for 2 moles of Al from the balanced equation

Calculating the energy from mass of Al (Al is 26.98 g/mol)

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Problem Details

How much energy is evolved during the reaction of 51.2 g of Al, according to the reaction below?

Assume that there is excess Fe2O3.

Fe2O3(s) + 2 Al(s) → Al2O3(s) + 2 Fe(s)          ΔH°rxn = -852 kJ 

A) 51.2 kJ 

B) 448 kJ 

C) 224 kJ 

D) 1617 kJ 

E) 808 kJ