The Ostwald process is used commercially to produce nitric acid, which is, in turn, used in many modern chemical processes. In the first step of the Ostwald process, ammonia is reacted with oxygen gas to produce nitric oxide and water. What is the maximum mass of H2O that can be produced by combining 90.1 g of each reactant?
The Ostwald process is used commercially to produce nitric acid, which is, in turn, used in many modern chemical processes. In the first step of the Ostwald process, ammonia is reacted with oxygen gas to produce nitric oxide and water. What is the maximum mass of H2O that can be produced by combining 90.1 g of each reactant?
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter4: Energy And Chemical Reactions
Section: Chapter Questions
Problem 57QRT
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The Ostwald process is used commercially to produce nitric acid, which is, in turn, used in many modern chemical processes. In the first step of the Ostwald process, ammonia is reacted with oxygen gas to produce nitric oxide and water.
What is the maximum mass of H2O that can be produced by combining 90.1 g of each reactant?
![**Chemical Reaction for the Combustion of Ammonia**
This equation represents the reaction between ammonia (NH₃) and oxygen (O₂) to form nitrogen monoxide (NO) and water (H₂O). It is an example of a chemical process involving gases:
\[ 4 \text{NH}_3 (g) + 5 \text{O}_2 (g) \rightarrow 4 \text{NO} (g) + 6 \text{H}_2\text{O} (g) \]
**Components and Coefficients:**
- **Reactants:**
- **Ammonia (NH₃):** 4 molecules
- **Oxygen (O₂):** 5 molecules
- **Products:**
- **Nitrogen Monoxide (NO):** 4 molecules
- **Water (H₂O):** 6 molecules
This balanced chemical reaction illustrates the stoichiometry of the process, showing the conservation of mass where the number of atoms for each element is equal on both sides of the equation.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fe3aa2ebc-6e44-4e1e-8169-ec975f43d301%2Fa964385b-3376-4e52-8760-be32c3ac4ff2%2Fkxzi9s_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Chemical Reaction for the Combustion of Ammonia**
This equation represents the reaction between ammonia (NH₃) and oxygen (O₂) to form nitrogen monoxide (NO) and water (H₂O). It is an example of a chemical process involving gases:
\[ 4 \text{NH}_3 (g) + 5 \text{O}_2 (g) \rightarrow 4 \text{NO} (g) + 6 \text{H}_2\text{O} (g) \]
**Components and Coefficients:**
- **Reactants:**
- **Ammonia (NH₃):** 4 molecules
- **Oxygen (O₂):** 5 molecules
- **Products:**
- **Nitrogen Monoxide (NO):** 4 molecules
- **Water (H₂O):** 6 molecules
This balanced chemical reaction illustrates the stoichiometry of the process, showing the conservation of mass where the number of atoms for each element is equal on both sides of the equation.
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