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)
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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