Aluminum is produced commercially by high-temperature electrolysis of aluminum oxide. When 1.500 x 10³ g of Al₂O₃ is reacted with excess C, 601 g of Al is produced. Calculate the percent yield for the production of Al.
Al₂O₃(s) + 3 C(s) $\rightarrow$ 2 Al(s) + 3 CO(g)

Question

Aluminum is produced commercially by high-temperature electrolysis of aluminum oxide. When 1.500 x 10³ g of Al₂O₃ is reacted with excess C, 601 g of Al is produced. Calculate the percent yield for the production of Al.
Al₂O₃(s) + 3 C(s)

\rightarrow

2 Al(s) + 3 CO(g)

Quizplus · Accepted Answer

The theoretical yield of Al can be calculated from the stoichiometry of the reaction. The molar mass of Al2O3 is 101.96 g/mol, and that of Al is 26.98 g/mol. From 1.500 x 10^3 g of Al2O3, the theoretical yield of Al is 2 x (1.500 x 10^3 g / 101.96 g/mol) x 26.98 g/mol = 795.6 g. The percent yield is (601 g / 795.6 g) x 100% = 75.7%.

Aluminum Is Produced Commercially by High-Temperature Electrolysis of Aluminum Oxide →\rightarrow→

Aluminum Is Produced Commercially by High-Temperature Electrolysis of Aluminum Oxide $\rightarrow$