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3. Ammonia (NH:) is produced by the equation below: N2 (g) + H2 (g) → NH3 (g) a) Balance the equation above b) How many grams of ammonia will be produced if 10 g of nitrogen gas reacts?

3. Ammonia (NH:) is produced by the equation below: N2 (g) + H2 (g) → NH3 (g) a) Balance the equation above b) How many grams of ammonia will be produced if 10 g of nitrogen gas reacts?

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
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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3. Ammonia (NH:) is produced by the equation below: N2 (g) + H2 (g) → NH3 (g) a) Balance the equation above b) How many grams of ammonia will be produced if 10 g of nitrogen gas reacts? c) If this reaction was performed in lab and generated 8.7 g of ammonia, calculate the percent yield for this experiment. 4. The combustion of methane gas (CH.) is shown in the reaction below: CH (g) + O2 (g) → CO2 (g) + H:O (g) If you burn 15 grams of methane with excess oxygen and form 28.4 grams of water, calculate the percent yield of water formed.
Transcribed Image Text:3. Ammonia (NH:) is produced by the equation below: N2 (g) + H2 (g) → NH3 (g) a) Balance the equation above b) How many grams of ammonia will be produced if 10 g of nitrogen gas reacts? c) If this reaction was performed in lab and generated 8.7 g of ammonia, calculate the percent yield for this experiment. 4. The combustion of methane gas (CH.) is shown in the reaction below: CH (g) + O2 (g) → CO2 (g) + H:O (g) If you burn 15 grams of methane with excess oxygen and form 28.4 grams of water, calculate the percent yield of water formed.
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