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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![### Formation of Solid Ammonium Chloride (NH₄Cl)
**Reaction Overview:**
Solid ammonium chloride, NH₄Cl, is formed by the reaction of gaseous ammonia, NH₃, and hydrogen chloride, HCl.
\[ \text{NH}_3 (g) + \text{HCl} (g) \rightarrow \text{NH}_4\text{Cl} (s) \]
**Experimental Setup:**
A 3.13 g sample of NH₃ gas and a 3.13 g sample of HCl gas are mixed in a 1.50 L flask at 25 °C.
#### Steps to Consider:
1. **Identify the Limiting Reagent:**
- This step involves determining which reactant will be completely consumed first in the reaction.
- Options:
- NH₄Cl
- HCl
- NH₃
2. **Calculate the Mass of NH₄Cl Formed:**
- Determine how many grams of NH₄Cl will be produced from the given amounts of NH₃ and HCl.
3. **Determine the Pressure of Remaining Gas:**
- Calculate the pressure (in atmospheres) of any gas remaining in the flask after the reaction.
- Note: Ignore the volume of solid NH₄Cl produced by the reaction.
**Questions and Calculation Requirements:**
1. **Identify the Limiting Reagent:**
- Choose the correct limiting reagent based on stoichiometric calculations.
2. **How many grams of NH₄Cl will be formed by this reaction?**
- Input the calculated mass:
\[
\text{mass}: \_\_\_\_\_\_\_\_ \text{g}
\]
3. **What is the pressure in atmospheres of the gas remaining in the flask?**
- Input the calculated pressure:
\[
P = \_\_\_\_\_\_\_\_ \text{atm}
\]
These steps guide you through the stoichiometric analysis and allow you to determine both the limiting reagent and the quantities involved in the formation of NH₄Cl. Ensure accurate calculations to find the correct reactant amounts and resulting pressures.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F5c433f37-c484-4136-9ada-41e91862a98c%2Fa1d1e701-0115-41fa-b938-150147dc08c0%2Fazf8xgr_processed.png&w=3840&q=75)
Transcribed Image Text:### Formation of Solid Ammonium Chloride (NH₄Cl)
**Reaction Overview:**
Solid ammonium chloride, NH₄Cl, is formed by the reaction of gaseous ammonia, NH₃, and hydrogen chloride, HCl.
\[ \text{NH}_3 (g) + \text{HCl} (g) \rightarrow \text{NH}_4\text{Cl} (s) \]
**Experimental Setup:**
A 3.13 g sample of NH₃ gas and a 3.13 g sample of HCl gas are mixed in a 1.50 L flask at 25 °C.
#### Steps to Consider:
1. **Identify the Limiting Reagent:**
- This step involves determining which reactant will be completely consumed first in the reaction.
- Options:
- NH₄Cl
- HCl
- NH₃
2. **Calculate the Mass of NH₄Cl Formed:**
- Determine how many grams of NH₄Cl will be produced from the given amounts of NH₃ and HCl.
3. **Determine the Pressure of Remaining Gas:**
- Calculate the pressure (in atmospheres) of any gas remaining in the flask after the reaction.
- Note: Ignore the volume of solid NH₄Cl produced by the reaction.
**Questions and Calculation Requirements:**
1. **Identify the Limiting Reagent:**
- Choose the correct limiting reagent based on stoichiometric calculations.
2. **How many grams of NH₄Cl will be formed by this reaction?**
- Input the calculated mass:
\[
\text{mass}: \_\_\_\_\_\_\_\_ \text{g}
\]
3. **What is the pressure in atmospheres of the gas remaining in the flask?**
- Input the calculated pressure:
\[
P = \_\_\_\_\_\_\_\_ \text{atm}
\]
These steps guide you through the stoichiometric analysis and allow you to determine both the limiting reagent and the quantities involved in the formation of NH₄Cl. Ensure accurate calculations to find the correct reactant amounts and resulting pressures.
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