Silver metal reacts with sulfur to form silver sulfide according to the following reaction: 2Ag(s) + S(s) – Ag2S(s) a. Identify the limiting reagent if 50.0 g Ag reacts with 10.0 g S b. What is the theoretical yield in g of Ag2S produced from the reaction? c. What is the amount in g of the excess reactant expected to remain after the reaction? d. When the reaction occurred, the amount of Ag2S obtained was 45.0 g. What is the percent yield of the reaction?
Silver metal reacts with sulfur to form silver sulfide according to the following reaction: 2Ag(s) + S(s) – Ag2S(s) a. Identify the limiting reagent if 50.0 g Ag reacts with 10.0 g S b. What is the theoretical yield in g of Ag2S produced from the reaction? c. What is the amount in g of the excess reactant expected to remain after the reaction? d. When the reaction occurred, the amount of Ag2S obtained was 45.0 g. What is the percent 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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