The reaction of aluminium and chlorine is illustrated by the following chemical equation: 2 Al (s) + 3 Cl2(g) → 2 AlCl3(s) (a) If 1.50 mol of Al reacts with 3.00 mol of Cl2(g), which reagent is the limiting reagent? (b) How many moles of AlCl3 are formed? (c) If 50.0 g of AlCl3 is formed in the reaction, what is the percentage yield?
The reaction of aluminium and chlorine is illustrated by the following chemical equation: 2 Al (s) + 3 Cl2(g) → 2 AlCl3(s) (a) If 1.50 mol of Al reacts with 3.00 mol of Cl2(g), which reagent is the limiting reagent? (b) How many moles of AlCl3 are formed? (c) If 50.0 g of AlCl3 is formed in the reaction, what is the percentage yield?
Chemistry for Engineering Students
4th Edition
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Lawrence S. Brown, Tom Holme
Chapter4: Stoichiometry
Section: Chapter Questions
Problem 4.44PAE: 4.44 Industrial production of hydrogen gas uses the reaction shown below. If 1.00 metric ton of...
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The reaction of aluminium and chlorine is illustrated by the following chemical equation:
2 Al (s) + 3 Cl2(g) → 2 AlCl3(s)
(a) If 1.50 mol of Al reacts with 3.00 mol of Cl2(g), which reagent is the
limiting reagent?
(b) How many moles of AlCl3 are formed?
(c) If 50.0 g of AlCl3 is formed in the reaction, what is the percentage yield?
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