🤓 Based on our data, we think this question is relevant for Professor Arnett's class at FAMU.
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