Thermite is a reaction that was once used to weld railroads together as shown below. A 48.0 g sample of Al(s) was reacted with 99.0 g of Fe₂O₃ according to the equation below. What could be the theoretical yield of Fe_(s) in grams?
2 Al_(s) + Fe₂O_3(s) $\rarr$ Al₂O_3(s)+ 2 Fe_(s)

Question

Thermite is a reaction that was once used to weld railroads together as shown below. A 48.0 g sample of Al(s) was reacted with 99.0 g of Fe₂O₃ according to the equation below. What could be the theoretical yield of Fe_(s) in grams?
2 Al_(s) + Fe₂O_3(s)

\rarr

Al₂O_3(s)+ 2 Fe_(s)

Quizplus · Accepted Answer

The balanced equation shows that 2 moles of Al react with 1 mole of Fe2O3 to produce 2 moles of Fe. Calculate moles of Al (48.0 g / 26.98 g/mol) and Fe2O3 (99.0 g / 159.69 g/mol). Al is the limiting reactant. Use stoichiometry to find moles of Fe produced and convert to grams (moles of Fe x 55.85 g/mol). The theoretical yield is approximately 69.2 g.

Thermite Is a Reaction That Was Once Used to Weld →\rarr→

Thermite Is a Reaction That Was Once Used to Weld $\rarr$