MODEL: GASES EXERT PRESSURE INDEPENDENTLY Condition Pressure initial final 1.0 atm 3.0 atm Volume 22.4 L 22.4 L Temperature 273 K 273 K Comment 1.0 mole of N₂ gas fills the tank. 2.0 moles of O2 gas have been added to the 1 mole of N₂ gas in the tank.
MODEL: GASES EXERT PRESSURE INDEPENDENTLY Condition Pressure initial final 1.0 atm 3.0 atm Volume 22.4 L 22.4 L Temperature 273 K 273 K Comment 1.0 mole of N₂ gas fills the tank. 2.0 moles of O2 gas have been added to the 1 mole of N₂ gas in the tank.
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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What amount of pressure do you think the nitrogen contributed to the final total pressure? Explain your reasoning.
Transcribed Image Text:**Model: Gases Exert Pressure Independently**
This table illustrates how gases behave when exerting pressure independently, using an example involving nitrogen (N₂) and oxygen (O₂) gases.
| Condition | Pressure | Volume | Temperature | Comment |
|-----------|----------|--------|-------------|---------|
| Initial | 1.0 atm | 22.4 L | 273 K | 1.0 mole of N₂ gas fills the tank. |
| Final | 3.0 atm | 22.4 L | 273 K | 2.0 moles of O₂ gas have been added to the 1 mole of N₂ gas in the tank. |
- **Initial Condition:** The tank is filled with 1.0 mole of nitrogen gas, resulting in a pressure of 1.0 atm at a volume of 22.4 liters and a temperature of 273 Kelvin.
- **Final Condition:** After adding 2.0 moles of oxygen gas to the existing nitrogen gas, the pressure increases to 3.0 atm. The volume and temperature remain constant at 22.4 liters and 273 Kelvin, respectively.
This demonstrates the principle that the total pressure is the sum of the partial pressures of individual gases in a mixture, illustrating Dalton's Law of Partial Pressures.
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