According to the following reaction, how many grams of dinitrogen monoxide will be formed upon the complete reaction of 21.0 grams of ammonium nitrate? NH,NO3 (aq) N2O (g) + 2H2O (1) grams dinitrogen monoxide
According to the following reaction, how many grams of dinitrogen monoxide will be formed upon the complete reaction of 21.0 grams of ammonium nitrate? NH,NO3 (aq) N2O (g) + 2H2O (1) grams dinitrogen monoxide
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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![**Problem Statement:**
According to the following reaction, how many grams of **dinitrogen monoxide** will be formed upon the complete reaction of 21.0 grams of **ammonium nitrate**?
\[ \text{NH}_4\text{NO}_3 (\text{aq}) \rightarrow \text{N}_2\text{O} (\text{g}) + 2\text{H}_2\text{O} (\text{l}) \]
**Answer Box:**
____ grams **dinitrogen monoxide**
**Explanation:**
This problem is an example of a stoichiometry calculation in chemistry. Given the reaction:
\[ \text{NH}_4\text{NO}_3 \rightarrow \text{N}_2\text{O} + 2\text{H}_2\text{O} \]
We need to calculate the mass of dinitrogen monoxide (\(\text{N}_2\text{O}\)) produced from a known mass of ammonium nitrate (\(\text{NH}_4\text{NO}_3\)).
To solve this, follow these steps:
1. **Determine the Molar Masses:**
- Ammonium Nitrate (\(\text{NH}_4\text{NO}_3\)): 80.04 g/mol
- Dinitrogen Monoxide (\(\text{N}_2\text{O}\)): 44.02 g/mol
2. **Convert Grams to Moles:**
- Moles of \(\text{NH}_4\text{NO}_3 = \frac{21.0 \text{ g}}{80.04 \text{ g/mol}}\)
3. **Use Stoichiometry:**
- The balanced equation shows a 1:1 molar ratio between \(\text{NH}_4\text{NO}_3\) and \(\text{N}_2\text{O}\).
- Moles of \(\text{N}_2\text{O}\) produced is equal to moles of \(\text{NH}_4\text{NO}_3\).
4. **Convert Moles to Grams:**
- Grams of \(\text{N}_2\text{O} = \text{Moles of } \text{N}_2\text{O} \times 44.02 \text](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fa6863c8d-f09e-486e-9969-ee798cd8c2b9%2F1e260a32-e3b7-43fd-82e1-b96aa4488060%2Fq1iwxfe_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Problem Statement:**
According to the following reaction, how many grams of **dinitrogen monoxide** will be formed upon the complete reaction of 21.0 grams of **ammonium nitrate**?
\[ \text{NH}_4\text{NO}_3 (\text{aq}) \rightarrow \text{N}_2\text{O} (\text{g}) + 2\text{H}_2\text{O} (\text{l}) \]
**Answer Box:**
____ grams **dinitrogen monoxide**
**Explanation:**
This problem is an example of a stoichiometry calculation in chemistry. Given the reaction:
\[ \text{NH}_4\text{NO}_3 \rightarrow \text{N}_2\text{O} + 2\text{H}_2\text{O} \]
We need to calculate the mass of dinitrogen monoxide (\(\text{N}_2\text{O}\)) produced from a known mass of ammonium nitrate (\(\text{NH}_4\text{NO}_3\)).
To solve this, follow these steps:
1. **Determine the Molar Masses:**
- Ammonium Nitrate (\(\text{NH}_4\text{NO}_3\)): 80.04 g/mol
- Dinitrogen Monoxide (\(\text{N}_2\text{O}\)): 44.02 g/mol
2. **Convert Grams to Moles:**
- Moles of \(\text{NH}_4\text{NO}_3 = \frac{21.0 \text{ g}}{80.04 \text{ g/mol}}\)
3. **Use Stoichiometry:**
- The balanced equation shows a 1:1 molar ratio between \(\text{NH}_4\text{NO}_3\) and \(\text{N}_2\text{O}\).
- Moles of \(\text{N}_2\text{O}\) produced is equal to moles of \(\text{NH}_4\text{NO}_3\).
4. **Convert Moles to Grams:**
- Grams of \(\text{N}_2\text{O} = \text{Moles of } \text{N}_2\text{O} \times 44.02 \text
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