How much energy is evolved during the formation of 98.7 g of Fe according to the reaction below? Fe₂O₃(s) + 2Al(s) → Al₂O₃(s) + 2Fe(s)
D_rH°= -852 kJ

Question

How much energy is evolved during the formation of 98.7 g of Fe according to the reaction below? Fe₂O₃(s)+ 2Al(s)→ Al₂O₃(s)+ 2Fe(s) D_rH°= -852 kJ

Quizplus · Accepted Answer

The molar mass of Fe is 55.85 g/mol, so 98.7 g of Fe is 1.77 mol. The reaction produces 2 mol of Fe per reaction, releasing 852 kJ. Therefore, 1.77 mol of Fe releases (1.77/2) * 852 kJ = 753 kJ.

How Much Energy Is Evolved During the Formation of 98