3. Aluminum does not occur naturally in its elemental form and therefore must be refined from ore. Part of this process involves the balanced reaction shown here. 2 Al2O3 + 3 C4 Al + 3 CO2 A production run utilizes 25.0 kg Al2O3 and 5.00 kg of carbon, and produces 9.47 kg of Al. a. Calculate the molar mass of Al2O3 (show your work here): b. Calculate the theoretical yield of Al in moles. This will require two stoichiometry calculations - one for each reactant. Show all work clearly. c. Limiting reactant: Excess reactant: d. Convert the theoretical yield (from part b) into kg of Al. Calculate the percent yield of this process.
3. Aluminum does not occur naturally in its elemental form and therefore must be refined from ore. Part of this process involves the balanced reaction shown here. 2 Al2O3 + 3 C4 Al + 3 CO2 A production run utilizes 25.0 kg Al2O3 and 5.00 kg of carbon, and produces 9.47 kg of Al. a. Calculate the molar mass of Al2O3 (show your work here): b. Calculate the theoretical yield of Al in moles. This will require two stoichiometry calculations - one for each reactant. Show all work clearly. c. Limiting reactant: Excess reactant: d. Convert the theoretical yield (from part b) into kg of Al. Calculate the percent yield of this process.
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter3: Stoichiometry
Section: Chapter Questions
Problem 182CP: The aspirin substitute, acetaminophen (C8H9O2N), is produced by the following three-step synthesis:...
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