11. How much aluminum can be produced from the \(1.00 \times 10^{3} \mathrm{~kg}\) mineral bauxite, which mostly \(\mathrm{Al}_{2} \mathrm{O}_{3} ?\)
Bauxite = Al2O3
The balanced reaction of production of Al from Al2O3
2Al2O3 = 4Al + 3O2
Mass of Al2O3 = 1.00*10^3 kg
Moles of Al2O3 = mass/molecular weight
= (1.00*10^3 kg) / (101.96 kg/kmol)
= 9.808 kmol
From the stoichiometry of the reaction
2 kmoles Al2O3 produces = 4 kmoles Al
9.808 kmol Al2O3 produces = 9.808*4/2 kmoles Al
= 19.616 kmol
Mass of Al = moles x molecular weight
= 19.616 kmol x 26.98 kg/kmol
= 529.23 kg
= 5.29 * 10^2 kg
Q11. Given : mass Al2O3 = 1.00 x 103 kg
mass Al2O3 = 1.00 x 103 kg * (1000 g / 1 kg)
mass Al2O3 = 1.00 x 106 g
moles Al2O3 = (mass Al2O3) / (molar mass Al2O3)
moles Al2O3 = (1.00 x 106 g) / (102 g/mol)
moles Al2O3 = 9803.9 mol
Al2O3 (s) 2 Al (s) + 3/2 O2 (g)
moles Al produced = 2 * (moles Al2O3)
moles Al produced = 2 * (9803.9 mol)
moles Al produced = 19607.8 mol
mass Al produced = (moles Al produced) * (molar mass Al)
mass Al produced = (19607.8 mol) * (27.0 g/mol)
mass Al produced = 529411.8 g
mass Al produced = 529411.8 g * (1 kg / 1000 g)
mass Al produced = 529 kg
11. How much aluminum can be produced from the 1.00 x 103 kg mineral bauxite, which...
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