The mineral bauxite, which is mostly Al2O3, is the principal industrial source of aluminum metal. How much aluminum can be produced from 4.50 ton of Al2O3
Since we know that
Molar mass of \(\mathrm{Al} 2 \mathrm{O} 3=101.96 \mathrm{~g} / \mathrm{mol}\)
The molar mass of \(\mathrm{Al}=26.98 \mathrm{~g} / \mathrm{mol}\)
1 mole of \(\mathrm{Al} 2 \mathrm{O} 3\) produces 2 moles of \(\mathrm{Al}\)
\(101.96 \mathrm{~g}\) of \(\mathrm{Al} 2 \mathrm{O} 3\) produces \(2 \times 26.98=53.96 \mathrm{~g}\) of \(\mathrm{Al}\)
Since we know that
\(1 \mathrm{~g}=1.102 \times 10^{-6}\) tons
then
\(101.96 \times 1.102 \times 10^{-6}\) tons of \(\mathrm{Al} 2 \mathrm{O} 3\) produces \(53.96 \times 1.102 \times 10^{-6}\) tons of \(\mathrm{Al}\)
4.50 tons of \(\mathrm{A} 12 \mathrm{O} 3\) produce \(\left(4.50 /\left(101.96 \times 1.102 \times 10^{-6}\right)\right) \times\left(53.96 \times 1.102 \times 10^{-6}\right)\)
\(=2.38\) tons of Al Answer
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, a mineral that is 75.0% Al2O3, by weight. How many kilograms of aluminum can be obtained from 100.00 kg of bauxite?
The aluminum in bauxite must be separated from its oxygen and hydrogen compounds and then further purified to produce the pure metal that we are all familiar with. A large amount of electrical energy is required to obtain pure aluminum metal. For example, processing 1 kg of aluminum from bauxite ore consumes 30 kwh of electricity. One of the most common uses of aluminum is for beverage cans. A standard size aluminum beverage can weigh 13 grams. Last year, the...
Aluminum is produced by electrolysis of molten Al2O3-Na3AlF6 mixture using a series of electrolytic cells that operates at a total voltage of 4.5 V and a constant current of 1.50 x 105 A? How many grams of aluminum can be produced per hour using the above amperage? How much energy (in kWhr) is consumed during the electrolysis? (Answer: 50.3 kg; 675 kWh)
The extraction of aluminum metal from the aluminum hydroxide found in bauxite by the Hall-Héroult process is one of the most remarkable success stories of 19th century chemistry, turning aluminum from a rare and precious metal into the cheap commodity it is today. In the first step, aluminum hydroxide reacts to form alumina Al2O3 and water: 2AlOH3(s)→ Al2O3(s)+ 3H2O(g) In the second step, alumina Al2O3 and carbon react to form aluminum and carbon dioxide: 2Al2O3(s)+ 3C(s)→ 4Al(s)+ 3CO2(g) Suppose the...
Iron metal can be produced by the reaction shown below. Calculate the mass of aluminum that is required to react completely with 345 g of Feo. 2 Al(s) + 3 FeO (s) 3 Fe (1) + Al2O3 (s) Write the answer in the space provided below and submit your calculations to show how you determined the answer in your work upload after the quiz. mass of aluminum: Iron metal can be produced by the reaction shown below. Calculate the mass...
How many grams of Al2O3 are produced if the reaction starts with 35.0 grams of aluminum? (Assume there is plenty of oxygen present.) 4 Al + 3 O2 → 2 ALO3 5.00 2.59 0.648 66.18
The extraction of aluminum metal from the aluminum hydroxide in bauxite ore by the Hall-Héroult process is one of the most remarkable success stories of late 19th century practical chemistry, turning aluminum from a rare and precious metal into the cheap commodity it is today. In the first step, aluminum hydroxide reacts to form alumina and water: 2AlOH3 (s) → Al2O3 (s) + 3H2O (g) In the second step, alumina and carbon react to form aluminum and carbon dioxide: 2Al2O3...
Differential Analysis Report for Further Processing The management of Dorsch Aluminum Co. is considering whether to process aluminum ingot further into rolled aluminum. Rolled aluminum can be sold for $4,480 per ton, and ingot can be sold without further processing for $2,508.8 per ton. Ingot is produced in batches of 110 tons by smelting 275 tons of bauxite, which costs $627.2 per ton. Rolled aluminum will require additional processing costs of $940.8 per ton of ingot, and 1.2 tons of...
Aluminum oxide (Al2O3) is produced according to the following equation. 4 Al(s) + 3 O2(g) → 2 Al2O3(s) If the reaction occurs with an 82.4% yield, what mass of aluminum should be reacted with excess oxygen to produce 45.0 grams of Al2O3? a. 54.6 g Al b. 37.9 g Al c. 35.1 g Al d. 23.8 g Al e. 28.9 g Al How do we solve this problem