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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![### Ideal Gas Law Problem: Determining Moles of Chlorine Gas
#### Problem Statement:
Calculate the number of moles of chlorine gas at a temperature of 120.0°C and a pressure of 26.1 bar, occupying a vessel with a volume of 31.0 L. Use the ideal gas constant \( R = 0.08314 \, \text{L} \cdot \text{bar/mol} \cdot \text{K} \).
#### Input Section:
Enter the calculated number of moles (mol) using the on-screen keypad. The keypad includes numbers 0-9, a decimal point, and options to multiply by 10 (\( x10 \)) or clear the entry.
### Explanation:
This task involves using the ideal gas law equation:
\[ PV = nRT \]
Where:
- \( P \) = Pressure (26.1 bar)
- \( V \) = Volume (31.0 L)
- \( n \) = Number of moles
- \( R \) = Ideal gas constant (\( 0.08314 \, \text{L} \cdot \text{bar/mol} \cdot \text{K} \))
- \( T \) = Temperature (in Kelvin; convert from Celsius by adding 273.15)
The equation rearranges to solve for moles (\( n \)) as follows:
\[ n = \frac{PV}{RT} \]
#### Steps:
1. **Convert Temperature**:
\[ T = 120.0^\circ\text{C} + 273.15 = 393.15 \, \text{K} \]
2. **Substitute Values**:
\[ n = \frac{26.1 \times 31.0}{0.08314 \times 393.15} \]
3. **Calculate the Result**:
- Perform the multiplication and division to find \( n \).
Use the keypad interface to input your calculated value and verify your result.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Ffa1d4005-1055-4b4d-a642-2588fc3ac80f%2Fe6ebba39-09b8-40e5-9f1b-bd11565426ee%2Fi5kmdxg_processed.png&w=3840&q=75)
Transcribed Image Text:### Ideal Gas Law Problem: Determining Moles of Chlorine Gas
#### Problem Statement:
Calculate the number of moles of chlorine gas at a temperature of 120.0°C and a pressure of 26.1 bar, occupying a vessel with a volume of 31.0 L. Use the ideal gas constant \( R = 0.08314 \, \text{L} \cdot \text{bar/mol} \cdot \text{K} \).
#### Input Section:
Enter the calculated number of moles (mol) using the on-screen keypad. The keypad includes numbers 0-9, a decimal point, and options to multiply by 10 (\( x10 \)) or clear the entry.
### Explanation:
This task involves using the ideal gas law equation:
\[ PV = nRT \]
Where:
- \( P \) = Pressure (26.1 bar)
- \( V \) = Volume (31.0 L)
- \( n \) = Number of moles
- \( R \) = Ideal gas constant (\( 0.08314 \, \text{L} \cdot \text{bar/mol} \cdot \text{K} \))
- \( T \) = Temperature (in Kelvin; convert from Celsius by adding 273.15)
The equation rearranges to solve for moles (\( n \)) as follows:
\[ n = \frac{PV}{RT} \]
#### Steps:
1. **Convert Temperature**:
\[ T = 120.0^\circ\text{C} + 273.15 = 393.15 \, \text{K} \]
2. **Substitute Values**:
\[ n = \frac{26.1 \times 31.0}{0.08314 \times 393.15} \]
3. **Calculate the Result**:
- Perform the multiplication and division to find \( n \).
Use the keypad interface to input your calculated value and verify your result.
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