1. Sixty grams of FeCl3 react with 50.0 g of H2S. 2FeCl3 + 3H2S → 6HCl + Fe2S3 a. What is the limiting reactant? b. What is the mass of HCl produced? c. What mass of excess reactant remains after the reaction? 2. 2Al + 3F2 → 2AlF3 In the reaction between aluminum and fluorine, 30.0 grams of the product is experimentally obtained when 0.45 mole of aluminum is used. Assuming that aluminum is the limiting reactant, calculate the percentage yield of the reaction.
1. Sixty grams of FeCl3 react with 50.0 g of H2S. 2FeCl3 + 3H2S → 6HCl + Fe2S3 a. What is the limiting reactant? b. What is the mass of HCl produced? c. What mass of excess reactant remains after the reaction? 2. 2Al + 3F2 → 2AlF3 In the reaction between aluminum and fluorine, 30.0 grams of the product is experimentally obtained when 0.45 mole of aluminum is used. Assuming that aluminum is the limiting reactant, calculate the percentage yield of the reaction.
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter3: Chemical Reactions
Section: Chapter Questions
Problem 121QRT: Ammonia can be formed by a direct reaction of nitrogen and hydrogen. N2(g) + 3 H2(g) 2 NH3(g) A...
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1. Sixty grams of FeCl3 react with 50.0 g of H2S.
2FeCl3 + 3H2S → 6HCl + Fe2S3
a. What is the limiting reactant?
b. What is the mass of HCl produced?
c. What mass of excess reactant remains after the reaction?
2. 2Al + 3F2 → 2AlF3
In the reaction between aluminum and fluorine, 30.0 grams of the product is experimentally obtained when 0.45 mole of aluminum is used. Assuming that aluminum is the limiting reactant, calculate the percentage yield of the reaction.
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