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5.78 Nitric acid is produced from nitrogen monoxide No which in turn is prepared from ammonia by the Ostwald process: 4NH3(g) + 502(g) → 4NO(g) + 6H,0(g) What volume of oxygen at 35°C and 2.15 atm is needed to produce 100.0 g of nitrogen monoxide?

5.78 Nitric acid is produced from nitrogen monoxide No which in turn is prepared from ammonia by the Ostwald process: 4NH3(g) + 502(g) → 4NO(g) + 6H,0(g) What volume of oxygen at 35°C and 2.15 atm is needed to produce 100.0 g of nitrogen monoxide?

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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**Chemistry Exercises on Gas Reactions and Balancing Equations** **5.77** Urea, NH₂CONH₂, is a nitrogen fertilizer that is manufactured from ammonia and carbon dioxide. \[ 2\text{NH}_3(g) + \text{CO}_2(g) \rightarrow \text{NH}_2\text{CONH}_2(s) + \text{H}_2\text{O}(l) \] *Question:* What volume of ammonia at 25°C and 4.00 atm is needed to produce 908 g (2 lb) of urea? --- **5.78** Nitric acid is produced from nitrogen monoxide, NO, which in turn is prepared from ammonia by the Ostwald process: \[ 4\text{NH}_3(g) + 5\text{O}_2(g) \rightarrow 4\text{NO}(g) + 6\text{H}_2\text{O}(g) \] *Question:* What volume of oxygen at 35°C and 2.15 atm is needed to produce 100.0 g of nitrogen monoxide? --- **5.79** Ammonium sulfate is used as a nitrogen and sulfur fertilizer. It is produced by reacting ammonia with sulfuric acid. *Task:* Write the balanced equation for the reaction of gaseous ammonia with sulfuric acid solution. What volume (in liters) of ammonia at 15°C and 1.15 atm is required to produce 150.0 g of ammonium sulfate? --- **5.80** Sodium hydrogen carbonate is also known as baking soda. When this compound is heated, it decomposes to sodium carbonate, carbon dioxide, and water vapor. *Task:* Write the balanced equation for this reaction. What volume (in liters) of carbon dioxide is produced at 100°C and 1.00 atm from the decomposition of 168 g of sodium hydrogen carbonate? --- These exercises involve chemical reactions, stoichiometry, and gas laws, focusing on the practical applications of fertilizers and everyday compounds like baking soda. Each problem requires a balanced chemical equation and calculations involving the ideal gas law to determine the volume of gases under specified conditions.
Transcribed Image Text:**Chemistry Exercises on Gas Reactions and Balancing Equations** **5.77** Urea, NH₂CONH₂, is a nitrogen fertilizer that is manufactured from ammonia and carbon dioxide. \[ 2\text{NH}_3(g) + \text{CO}_2(g) \rightarrow \text{NH}_2\text{CONH}_2(s) + \text{H}_2\text{O}(l) \] *Question:* What volume of ammonia at 25°C and 4.00 atm is needed to produce 908 g (2 lb) of urea? --- **5.78** Nitric acid is produced from nitrogen monoxide, NO, which in turn is prepared from ammonia by the Ostwald process: \[ 4\text{NH}_3(g) + 5\text{O}_2(g) \rightarrow 4\text{NO}(g) + 6\text{H}_2\text{O}(g) \] *Question:* What volume of oxygen at 35°C and 2.15 atm is needed to produce 100.0 g of nitrogen monoxide? --- **5.79** Ammonium sulfate is used as a nitrogen and sulfur fertilizer. It is produced by reacting ammonia with sulfuric acid. *Task:* Write the balanced equation for the reaction of gaseous ammonia with sulfuric acid solution. What volume (in liters) of ammonia at 15°C and 1.15 atm is required to produce 150.0 g of ammonium sulfate? --- **5.80** Sodium hydrogen carbonate is also known as baking soda. When this compound is heated, it decomposes to sodium carbonate, carbon dioxide, and water vapor. *Task:* Write the balanced equation for this reaction. What volume (in liters) of carbon dioxide is produced at 100°C and 1.00 atm from the decomposition of 168 g of sodium hydrogen carbonate? --- These exercises involve chemical reactions, stoichiometry, and gas laws, focusing on the practical applications of fertilizers and everyday compounds like baking soda. Each problem requires a balanced chemical equation and calculations involving the ideal gas law to determine the volume of gases under specified conditions.
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