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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![Title: Gas Laws and Quantitative Analysis
**Exercise: Calculating the Quantity in Moles of Chlorine Gas**
**Question:**
What quantity in moles of chlorine gas at 120.0°C and 33.3 atm would occupy a vessel of 26.5 L?
**Workspace:**
(unit: mol)
[Display of a digital calculator interface showing numerical input options and calculation commands]
**Instructions:**
Using the Ideal Gas Law, calculate the number of moles (\( n \)) of chlorine gas. Recall the Ideal Gas Law formula:
\[ PV = nRT \]
where:
- \( P \) is the pressure (in atm),
- \( V \) is the volume (in L),
- \( n \) is the number of moles,
- \( R \) is the ideal gas constant (0.0821 L·atm/(K·mol)),
- \( T \) is the temperature (in K).
1. Convert the given temperature from Celsius to Kelvin:
\[ T(K) = T(°C) + 273.15 = 120.0 + 273.15 = 393.15 \, K \]
2. Substitute the values into the Ideal Gas Law equation:
\[ (33.3 \, \text{atm})(26.5 \, \text{L}) = n(0.0821 \, \text{L·atm/(K·mol)})(393.15 \, \text{K}) \]
3. Solve for \( n \) (the number of moles):
\[ n = \frac{(33.3 \, \text{atm})(26.5 \, \text{L})}{(0.0821 \, \text{L·atm/(K·mol)})(393.15 \, \text{K})} \]
Use the calculator interface to perform the arithmetic operations step-by-step.
**Notes:**
- Double-check unit conversions and the value of the gas constant used.
- Ensure accuracy by carefully performing each arithmetic step.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F6895f9cd-8521-4c9a-bc62-df11c4ac3cae%2F7a36b2fc-2185-4eb7-8e12-178a0a4383bb%2F48nqius_processed.jpeg&w=3840&q=75)
Transcribed Image Text:Title: Gas Laws and Quantitative Analysis
**Exercise: Calculating the Quantity in Moles of Chlorine Gas**
**Question:**
What quantity in moles of chlorine gas at 120.0°C and 33.3 atm would occupy a vessel of 26.5 L?
**Workspace:**
(unit: mol)
[Display of a digital calculator interface showing numerical input options and calculation commands]
**Instructions:**
Using the Ideal Gas Law, calculate the number of moles (\( n \)) of chlorine gas. Recall the Ideal Gas Law formula:
\[ PV = nRT \]
where:
- \( P \) is the pressure (in atm),
- \( V \) is the volume (in L),
- \( n \) is the number of moles,
- \( R \) is the ideal gas constant (0.0821 L·atm/(K·mol)),
- \( T \) is the temperature (in K).
1. Convert the given temperature from Celsius to Kelvin:
\[ T(K) = T(°C) + 273.15 = 120.0 + 273.15 = 393.15 \, K \]
2. Substitute the values into the Ideal Gas Law equation:
\[ (33.3 \, \text{atm})(26.5 \, \text{L}) = n(0.0821 \, \text{L·atm/(K·mol)})(393.15 \, \text{K}) \]
3. Solve for \( n \) (the number of moles):
\[ n = \frac{(33.3 \, \text{atm})(26.5 \, \text{L})}{(0.0821 \, \text{L·atm/(K·mol)})(393.15 \, \text{K})} \]
Use the calculator interface to perform the arithmetic operations step-by-step.
**Notes:**
- Double-check unit conversions and the value of the gas constant used.
- Ensure accuracy by carefully performing each arithmetic step.
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