How much energy (kJ) is released when 15.0g of Fe(l) is produced in the thermite reaction
2Al(s) + Fe₂O₃(s) $\rarr$ Al₂O₃(s) + 2Fe(l) $\Delta$ H^$\circ$ = - 822.8 kJ/mol

Question

How much energy (kJ) is released when 15.0g of Fe(l) is produced in the thermite reaction 2Al(s) + Fe₂O₃(s) $\rarr$Al₂O₃(s) + 2Fe(l) $\Delta$H^$\circ$ = - 822.8 kJ/mol

Quizplus · Accepted Answer

The molar mass of Fe is 55.85 g/mol. For 15.0 g of Fe, the moles of Fe are 15.0 g / 55.85 g/mol = 0.2685 mol. Since the reaction produces 2 moles of Fe per reaction, the energy released is (0.2685 mol / 2) * 822.8 kJ/mol = 110. kJ.

How Much Energy (KJ) Is Released When 15 →\rarr→ Al2O3(s) + 2Fe(l)

How Much Energy (KJ) Is Released When 15 $\rarr$ Al₂O₃(s) + 2Fe(l)