How much energy (kJ)is released if 10.0g of Al(s)is reacted with excess Fe₂O₃(s)in the thermite reaction: 2Al(s)+ Fe₂O₃(s)$\rarr$ Al₂O₃(s)+ 2Fe(l)$\Delta$H° = - 822.8 kJ/mol

Question

Quizplus · Accepted Answer

The molar mass of Al is 26.98 g/mol. For 10.0 g of Al, moles = 10.0 g / 26.98 g/mol = 0.3707 mol. The reaction releases 822.8 kJ per 2 moles of Al, so for 0.3707 mol, energy released = 0.3707 mol * (822.8 kJ / 2 mol) = 152 kJ.

How Much Energy (KJ)is Released If 10 →\rarr→ Al2O3(s)+ 2Fe(l) Δ\DeltaΔ H° = - 822

How Much Energy (KJ)is Released If 10 $\rarr$ Al₂O₃(s)+ 2Fe(l) $\Delta$ H° = - 822