20. Gaseous ammonia reacts with chlorine gas to produce nitrogen gas and hydrogen chloride. What temperature is reached when 95.0 g of gaseous ammonia are reacted producing 30.0 L of hydrogen chloride at 850. torr?
20. Gaseous ammonia reacts with chlorine gas to produce nitrogen gas and hydrogen chloride. What temperature is reached when 95.0 g of gaseous ammonia are reacted producing 30.0 L of hydrogen chloride at 850. torr?
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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![### Chemistry Problem: Gas Reactions and Temperature Determination
**Problem Statement:**
20. Gaseous ammonia reacts with chlorine gas to produce nitrogen gas and hydrogen chloride. What temperature is reached when 95.0 g of gaseous ammonia are reacted producing 30.0 L of hydrogen chloride at 850. torr?
---
**Detailed Explanation:**
In this problem, we need to determine the temperature at which a reaction occurs, given certain conditions. The reaction involves gaseous ammonia (NH₃) and chlorine gas (Cl₂), which react to produce nitrogen gas (N₂) and hydrogen chloride (HCl).
**Steps to Solve the Problem:**
1. **Identify the Balanced Chemical Equation:**
\[
2 \text{NH}_3(g) + 3 \text{Cl}_2(g) \rightarrow \text{N}_2(g) + 6 \text{HCl}(g)
\]
2. **Convert Mass of Ammonia to Moles:**
\[
\text{Moles of NH}_3 = \frac{95.0 \text{ g}}{\text{Molar Mass of NH}_3}
\]
The molar mass of NH₃ (NH₃ = N + 3H) = 14 + (3 × 1) = 17 g/mol.
\[
\text{Moles of NH}_3 = \frac{95.0 \text{ g}}{17 \text{ g/mol}} \approx 5.59 \text{ moles}
\]
3. **Determine the Stoichiometric Relationship:**
From the balanced equation, 2 moles of NH₃ produce 6 moles of HCl. So, for 5.59 moles of NH₃:
\[
\text{Moles of HCl} = 5.59 \text{ moles NH}_3 \times \frac{6 \text{ moles HCl}}{2 \text{ moles NH}_3} = 16.77 \text{ moles HCl}
\]
4. **Use the Ideal Gas Law to Find the Temperature:**
The ideal gas law is given by \( PV = nRT \).
Convert the pressure from torr to atm:
\[
850 \text{ torr} \times \frac{](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fec9904e6-dc28-47e5-ba82-a0b2892d5fea%2F46dd9c18-b511-49da-beb6-7b6b0ad1c101%2Fknsigk_processed.png&w=3840&q=75)
Transcribed Image Text:### Chemistry Problem: Gas Reactions and Temperature Determination
**Problem Statement:**
20. Gaseous ammonia reacts with chlorine gas to produce nitrogen gas and hydrogen chloride. What temperature is reached when 95.0 g of gaseous ammonia are reacted producing 30.0 L of hydrogen chloride at 850. torr?
---
**Detailed Explanation:**
In this problem, we need to determine the temperature at which a reaction occurs, given certain conditions. The reaction involves gaseous ammonia (NH₃) and chlorine gas (Cl₂), which react to produce nitrogen gas (N₂) and hydrogen chloride (HCl).
**Steps to Solve the Problem:**
1. **Identify the Balanced Chemical Equation:**
\[
2 \text{NH}_3(g) + 3 \text{Cl}_2(g) \rightarrow \text{N}_2(g) + 6 \text{HCl}(g)
\]
2. **Convert Mass of Ammonia to Moles:**
\[
\text{Moles of NH}_3 = \frac{95.0 \text{ g}}{\text{Molar Mass of NH}_3}
\]
The molar mass of NH₃ (NH₃ = N + 3H) = 14 + (3 × 1) = 17 g/mol.
\[
\text{Moles of NH}_3 = \frac{95.0 \text{ g}}{17 \text{ g/mol}} \approx 5.59 \text{ moles}
\]
3. **Determine the Stoichiometric Relationship:**
From the balanced equation, 2 moles of NH₃ produce 6 moles of HCl. So, for 5.59 moles of NH₃:
\[
\text{Moles of HCl} = 5.59 \text{ moles NH}_3 \times \frac{6 \text{ moles HCl}}{2 \text{ moles NH}_3} = 16.77 \text{ moles HCl}
\]
4. **Use the Ideal Gas Law to Find the Temperature:**
The ideal gas law is given by \( PV = nRT \).
Convert the pressure from torr to atm:
\[
850 \text{ torr} \times \frac{
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