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 & Chemical Reactivity
9th Edition
ISBN:9781133949640
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter5: Principles Of Chemical Reactivity: Energy And Chemical Reactions
Section: Chapter Questions
Problem 120SCQ: In the reaction of two moles of gaseous hydrogen and one mole of gaseous oxygen to form two moles of...
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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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