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Silver metal reacts with sulfur to form silver sulfide according to the following reaction: 2Ag(s) + S(s) → Ag,S(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? Step 1. Analyze the problem. Step 2. Determine the limiting reagent. Step 3. Compute the theoretical yield. Step 4. Compute the percent yield.

Silver metal reacts with sulfur to form silver sulfide according to the following reaction: 2Ag(s) + S(s) → Ag,S(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? Step 1. Analyze the problem. Step 2. Determine the limiting reagent. Step 3. Compute the theoretical yield. Step 4. Compute the percent yield.

Chemistry
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
Chapter1: Chemical Foundations
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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 ing 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? Step 1. Analyze the problem. Step 2. Determine the limiting reagent. Step 3. Compute the theoretical yield. Step 4. Compute the percent yield.
Transcribed Image Text: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 ing 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? Step 1. Analyze the problem. Step 2. Determine the limiting reagent. Step 3. Compute the theoretical yield. Step 4. Compute the percent yield.
Silver metal reacts with sulfur to form silver sulfide according to the following reaction: 2Ag(s) + S(s) –→ Ag,S(s) Step 3. Compute the theoretical yield. Step 4. Compute the percent yield.
Transcribed Image Text:Silver metal reacts with sulfur to form silver sulfide according to the following reaction: 2Ag(s) + S(s) –→ Ag,S(s) Step 3. Compute the theoretical yield. Step 4. Compute the percent yield.
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