Ammonia, NH3, is produced at high temperatures and pressures in the presence of a catalyst as shown in the balanced equation below. N2 (g) + 3H2 (g) → 2NH3 (g) In an experiment 1250 grams of nitrogen were mixed with 5950 grams of hydrogen. 1. Find the theoretical yield in moles (or grams) assuming all of a given reactant reacted a. What is the theoretical yield of ammonia in moles if all the nitrogen reacted? (answer: 89.3 mol NH3) b. What is the theoretical yield of ammonia in moles if all the hydrogen reacted? (Answer: 1980 mol NH3) 2. Be able to identify the limiting and éxcess reactant. a. What is the NAME of the limiting reactant? (answer: nitrogen) b. What is the name of the excess reactant? (answer: hydrogen) 3. Calculate the theoretical yield of product based on the limiting reactant. a. What is the theoretical yield of ammonia in grams based on the limiting reactant? (1520 grams) 4. Calculate percent yield. a. What is the percent yield if the actual yield of ammonia was 1000. grams? (answer: 65.8%) 5. Calculate the amount of excess reactant left over after the reaction. a. How many grams of excess reactant remain after the reaction? (answer: 268 grams of H2 consumed therefore 5680 g excess H2)
Ammonia, NH3, is produced at high temperatures and pressures in the presence of a catalyst as shown in the balanced equation below. N2 (g) + 3H2 (g) → 2NH3 (g) In an experiment 1250 grams of nitrogen were mixed with 5950 grams of hydrogen. 1. Find the theoretical yield in moles (or grams) assuming all of a given reactant reacted a. What is the theoretical yield of ammonia in moles if all the nitrogen reacted? (answer: 89.3 mol NH3) b. What is the theoretical yield of ammonia in moles if all the hydrogen reacted? (Answer: 1980 mol NH3) 2. Be able to identify the limiting and éxcess reactant. a. What is the NAME of the limiting reactant? (answer: nitrogen) b. What is the name of the excess reactant? (answer: hydrogen) 3. Calculate the theoretical yield of product based on the limiting reactant. a. What is the theoretical yield of ammonia in grams based on the limiting reactant? (1520 grams) 4. Calculate percent yield. a. What is the percent yield if the actual yield of ammonia was 1000. grams? (answer: 65.8%) 5. Calculate the amount of excess reactant left over after the reaction. a. How many grams of excess reactant remain after the reaction? (answer: 268 grams of H2 consumed therefore 5680 g excess H2)
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
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Transcribed Image Text:Ammonia, NH3, is produced at high temperatures and pressures in the presence of a catalyst as
shown in the balanced equation below.
N2 (g)
+ 3H2 (g) >
2NH3 (g)
In an experiment 1250 grams of nitrogen were mixed with 5950 grams of hydrogen.
1. Find the theoretical yield in moles (or grams) assuming all of a given reactant reacted
a. What is the theoretical yield of ammonia in moles if all the nitrogen reacted?
(answer: 89.3 mol NH3)
b. What is the theoretical yield of ammonia in moles if all the hydrogen reacted?
(Answer: 1980 mol NH3)
2. Be able to identify the limiting and éxcess reactant.
a. What is the NAME of the limiting reactant? (answer: nitrogen)
b. What is the name of the excess reactant? (answer: hydrogen)
3. Calculate the theoretical yield of product based on the limiting reactant.
a. What is the theoretical yield of ammonia in grams based on the limiting
reactant? (1520 grams)
4. Calculate percent yield.
a. What is the percent yield if the actual yield of ammonia was 1000. grams?
(answer: 65.8%)
5. Calculate the amount of excess reactant left over after the reaction.
a. How many grams of excess reactant remain after the reaction?
(answer: 268 grams of H2 consumed therefore 5680 g excess H2)
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