Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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![### Ideal and Real Gases: Van der Waals Equation Application
According to the ideal gas law, a 1.008 mol sample of oxygen gas in a 1.684 L container at 269.7 K should exert a pressure of 13.25 atm. What is the percent difference between the pressure calculated using the van der Waals equation and the ideal pressure? For \( \text{O}_2 \) gas, \( a = 1.360 \, \frac{L^2 \cdot atm}{mol^2} \) and \( b = 0.03183 \, \frac{L}{mol} \).
#### Formula for Percent Difference
\[
\text{Percent difference} = \left( \frac{|P_{ideal} - P_{van \, der \, Waals}|}{\left( \frac{P_{ideal} + P_{van \, der \, Waals}}{2} \right)} \right) \times 100
\]
#### Calculation Box
Percent difference = \([ \text{Enter Value Here} ]\%\)
In this task, you will need to use the given constants for \( \text{O}_2 \) gas and calculate the pressure using both methods to find the percent difference.
This involves comparing the pressures obtained from the ideal gas law with those calculated using the Van der Waals equation, accounting for real gas behavior due to molecular interactions and volume.](https://content.bartleby.com/qna-images/question/e0f1975b-ad07-4857-b626-1368fa1e7067/b3c69f88-7f4e-4827-afee-8ded5a5bc0bc/edcaxr_processed.png)
Transcribed Image Text:### Ideal and Real Gases: Van der Waals Equation Application
According to the ideal gas law, a 1.008 mol sample of oxygen gas in a 1.684 L container at 269.7 K should exert a pressure of 13.25 atm. What is the percent difference between the pressure calculated using the van der Waals equation and the ideal pressure? For \( \text{O}_2 \) gas, \( a = 1.360 \, \frac{L^2 \cdot atm}{mol^2} \) and \( b = 0.03183 \, \frac{L}{mol} \).
#### Formula for Percent Difference
\[
\text{Percent difference} = \left( \frac{|P_{ideal} - P_{van \, der \, Waals}|}{\left( \frac{P_{ideal} + P_{van \, der \, Waals}}{2} \right)} \right) \times 100
\]
#### Calculation Box
Percent difference = \([ \text{Enter Value Here} ]\%\)
In this task, you will need to use the given constants for \( \text{O}_2 \) gas and calculate the pressure using both methods to find the percent difference.
This involves comparing the pressures obtained from the ideal gas law with those calculated using the Van der Waals equation, accounting for real gas behavior due to molecular interactions and volume.
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