### Problem Statement **Chemistry Problem: Stoichiometry and Molar Mass Calculations** **Objective:** Determine the grams of solid ammonium sulfate \((NH_4)_2SO_4\) produced. **Scenario:** Given the chemical reaction: \[2NH_3(g) + H_2SO_4(aq) \rightarrow (NH_4)_2SO_4(s)\] Calculate the mass of ammonium sulfate produced when: - 0.500 L of gaseous ammonia \((NH_3)\) reacts with an excess of sulfuric acid \((H_2SO_4)\). - Molar masses: - Ammonium sulfate \((NH_4)_2SO_4\) : 132.1 g/mol - Ammonia \((NH_3)\) : 17.0 g/mol - Sulfuric acid \((H_2SO_4)\) : 98.1 g/mol - Conditions: Standard Temperature and Pressure (STP) **Possible Answers:** - 77.7 g - 50.9 g - 19.4 g - 14.7 g ### Detailed Diagram Explanation The given chemical reaction represents the formation of solid ammonium sulfate from gaseous ammonia and aqueous sulfuric acid. ### Steps to Solve: 1. **Calculate Moles of Ammonia**: \[ \text{At STP, 1 mole of gas occupies 22.4 L} \\ \text{Given volume of NH}_3 = 0.500 \, \text{L} \] \[ \text{Moles of NH}_3 = \frac{0.500 \, \text{L}}{22.4 \, \text{L/mol}} = 0.0223 \, \text{mol} \] 2. **Use Stoichiometry to Determine Moles of Ammonium Sulfate**: \[ \text{From the reaction:} \quad 2 \, \text{moles of } NH_3 \text{ produce} 1 \, \text{mole of} \, (NH_4)_2SO_4 \\ \text{Moles of} \, (NH_4)_2SO_4 = \frac{0.022
### Problem Statement **Chemistry Problem: Stoichiometry and Molar Mass Calculations** **Objective:** Determine the grams of solid ammonium sulfate \((NH_4)_2SO_4\) produced. **Scenario:** Given the chemical reaction: \[2NH_3(g) + H_2SO_4(aq) \rightarrow (NH_4)_2SO_4(s)\] Calculate the mass of ammonium sulfate produced when: - 0.500 L of gaseous ammonia \((NH_3)\) reacts with an excess of sulfuric acid \((H_2SO_4)\). - Molar masses: - Ammonium sulfate \((NH_4)_2SO_4\) : 132.1 g/mol - Ammonia \((NH_3)\) : 17.0 g/mol - Sulfuric acid \((H_2SO_4)\) : 98.1 g/mol - Conditions: Standard Temperature and Pressure (STP) **Possible Answers:** - 77.7 g - 50.9 g - 19.4 g - 14.7 g ### Detailed Diagram Explanation The given chemical reaction represents the formation of solid ammonium sulfate from gaseous ammonia and aqueous sulfuric acid. ### Steps to Solve: 1. **Calculate Moles of Ammonia**: \[ \text{At STP, 1 mole of gas occupies 22.4 L} \\ \text{Given volume of NH}_3 = 0.500 \, \text{L} \] \[ \text{Moles of NH}_3 = \frac{0.500 \, \text{L}}{22.4 \, \text{L/mol}} = 0.0223 \, \text{mol} \] 2. **Use Stoichiometry to Determine Moles of Ammonium Sulfate**: \[ \text{From the reaction:} \quad 2 \, \text{moles of } NH_3 \text{ produce} 1 \, \text{mole of} \, (NH_4)_2SO_4 \\ \text{Moles of} \, (NH_4)_2SO_4 = \frac{0.022
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
**Chemistry Problem: Stoichiometry and Molar Mass Calculations**
**Objective:** Determine the grams of solid ammonium sulfate \((NH_4)_2SO_4\) produced.
**Scenario:**
Given the chemical reaction:
\[2NH_3(g) + H_2SO_4(aq) \rightarrow (NH_4)_2SO_4(s)\]
Calculate the mass of ammonium sulfate produced when:
- 0.500 L of gaseous ammonia \((NH_3)\) reacts with an excess of sulfuric acid \((H_2SO_4)\).
- Molar masses:
- Ammonium sulfate \((NH_4)_2SO_4\) : 132.1 g/mol
- Ammonia \((NH_3)\) : 17.0 g/mol
- Sulfuric acid \((H_2SO_4)\) : 98.1 g/mol
- Conditions: Standard Temperature and Pressure (STP)
**Possible Answers:**
- 77.7 g
- 50.9 g
- 19.4 g
- 14.7 g
### Detailed Diagram Explanation
The given chemical reaction represents the formation of solid ammonium sulfate from gaseous ammonia and aqueous sulfuric acid.
### Steps to Solve:
1. **Calculate Moles of Ammonia**:
\[
\text{At STP, 1 mole of gas occupies 22.4 L} \\
\text{Given volume of NH}_3 = 0.500 \, \text{L}
\]
\[
\text{Moles of NH}_3 = \frac{0.500 \, \text{L}}{22.4 \, \text{L/mol}} = 0.0223 \, \text{mol}
\]
2. **Use Stoichiometry to Determine Moles of Ammonium Sulfate**:
\[
\text{From the reaction:} \quad 2 \, \text{moles of } NH_3 \text{ produce} 1 \, \text{mole of} \, (NH_4)_2SO_4 \\
\text{Moles of} \, (NH_4)_2SO_4 = \frac{0.022](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F1be645a2-1b37-480f-ac5f-87052d4711ee%2Fc0381094-5802-41a9-9246-71f927448d31%2Fbm63b38_processed.jpeg&w=3840&q=75)
Transcribed Image Text:### Problem Statement
**Chemistry Problem: Stoichiometry and Molar Mass Calculations**
**Objective:** Determine the grams of solid ammonium sulfate \((NH_4)_2SO_4\) produced.
**Scenario:**
Given the chemical reaction:
\[2NH_3(g) + H_2SO_4(aq) \rightarrow (NH_4)_2SO_4(s)\]
Calculate the mass of ammonium sulfate produced when:
- 0.500 L of gaseous ammonia \((NH_3)\) reacts with an excess of sulfuric acid \((H_2SO_4)\).
- Molar masses:
- Ammonium sulfate \((NH_4)_2SO_4\) : 132.1 g/mol
- Ammonia \((NH_3)\) : 17.0 g/mol
- Sulfuric acid \((H_2SO_4)\) : 98.1 g/mol
- Conditions: Standard Temperature and Pressure (STP)
**Possible Answers:**
- 77.7 g
- 50.9 g
- 19.4 g
- 14.7 g
### Detailed Diagram Explanation
The given chemical reaction represents the formation of solid ammonium sulfate from gaseous ammonia and aqueous sulfuric acid.
### Steps to Solve:
1. **Calculate Moles of Ammonia**:
\[
\text{At STP, 1 mole of gas occupies 22.4 L} \\
\text{Given volume of NH}_3 = 0.500 \, \text{L}
\]
\[
\text{Moles of NH}_3 = \frac{0.500 \, \text{L}}{22.4 \, \text{L/mol}} = 0.0223 \, \text{mol}
\]
2. **Use Stoichiometry to Determine Moles of Ammonium Sulfate**:
\[
\text{From the reaction:} \quad 2 \, \text{moles of } NH_3 \text{ produce} 1 \, \text{mole of} \, (NH_4)_2SO_4 \\
\text{Moles of} \, (NH_4)_2SO_4 = \frac{0.022
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