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1. Matter and Measurements4h 31m
2. Atoms and the Periodic Table5h 23m
3. Ionic Compounds2h 18m
4. Molecular Compounds2h 18m
5. Classification & Balancing of Chemical Reactions3h 17m
6. Chemical Reactions & Quantities2h 27m
7. Energy, Rate and Equilibrium3h 46m
8. Gases, Liquids and Solids3h 25m
9. Solutions4h 10m
10. Acids and Bases3h 29m
11. Nuclear Chemistry56m
BONUS: Lab Techniques and Procedures1h 38m
BONUS: Mathematical Operations and Functions47m
12. Introduction to Organic Chemistry1h 34m
13. Alkenes, Alkynes, and Aromatic Compounds2h 12m
14. Compounds with Oxygen or Sulfur1h 6m
15. Aldehydes and Ketones1h 1m
16. Carboxylic Acids and Their Derivatives1h 11m
17. Amines39m
18. Amino Acids and Proteins1h 51m
19. Enzymes1h 37m
20. Carbohydrates1h 41m
21. The Generation of Biochemical Energy2h 8m
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23. Lipids2h 26m
24. Lipid Metabolism1h 45m
25. Protein and Amino Acid Metabolism1h 37m
26. Nucleic Acids and Protein Synthesis2h 54m

8. Gases, Liquids and Solids

Dalton's Law: Partial Pressure (Simplified)

GOB Chemistry

8. Gases, Liquids and Solids

Dalton's Law: Partial Pressure (Simplified)

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1:39 minutes

Problem 86

Textbook Question

What is meant by partial pressure?

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Partial pressure refers to the pressure exerted by a single gas in a mixture of gases. It is the contribution of that specific gas to the total pressure of the gas mixture.

The concept of partial pressure is based on Dalton's Law of Partial Pressures, which states that the total pressure of a gas mixture is the sum of the partial pressures of all the individual gases in the mixture.

Mathematically, Dalton's Law can be expressed as:

P_{total} = P_{1} + P_{2} + P_{3} + ...

, where Ptotal is the total pressure and P1, P2, etc., are the partial pressures of the individual gases.

To calculate the partial pressure of a gas, you can use the formula:

P_{gas} = X P_{total}

, where

X

is the mole fraction of the gas in the mixture.

Understanding partial pressure is important in various applications, such as gas exchange in the lungs, chemical reactions involving gases, and determining the behavior of gases under different conditions.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Partial Pressure

Partial pressure refers to the pressure exerted by a single component of a gas mixture. It is a fundamental concept in gas laws, indicating how much pressure a specific gas contributes to the total pressure of the mixture. This concept is crucial for understanding behaviors of gases in various conditions, such as in chemical reactions or biological systems.

Dalton's Law of Partial Pressures

Dalton's Law states that the total pressure of a gas mixture is equal to the sum of the partial pressures of its individual gases. This principle allows for the calculation of the contribution of each gas in a mixture, facilitating predictions about gas behavior under different conditions. It is essential in fields like chemistry, physics, and environmental science.

Gas Mixtures

Gas mixtures consist of two or more gases that can interact but maintain their individual properties. Understanding gas mixtures is vital for applications in various scientific fields, including atmospheric science and respiratory physiology. The behavior of these mixtures can be analyzed using concepts like partial pressure and Dalton's Law, which help in predicting how gases will react or behave in different environments.

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A mixture of nitrogen (N₂) and helium has a volume of 250 mL at 30 °C and a total pressure of 745 mmHg.

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What is the total pressure, in millimeters of mercury, of a gas mixture containing argon gas at 0.25 atm, helium gas at 350 mmHg, and nitrogen gas at 360 Torr?

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A mixture of nitrogen (N₂) and helium has a volume of 365 mL at 30 °C and a total pressure of 745 mmHg. (8.5, 8.6, 8.7)

a. If the partial pressure of helium is 65 mmHg, what is the partial pressure of the nitrogen?

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Multiple Choice

A gas mixture contains 72.8% chlorine and 27.2% neon by mass. What is the partial pressure of neon in the mixture if the total pressure is recorded as 809 mmHg?

The partial pressure of N₂ in the air is 593 mmHg at 1 atm. What is the partial pressure of N₂ in a bubble of air a scuba diver breathes when he is 66 ft below the surface of the water where the pressure is 3.00 atm?

Determine the percent composition of air in the lungs from the following composition in partial pressures: PN₂= 573 mmHg, PO₂ = 100 mmHg, PCO₂ = 40 mmHg, and PH₂O = 47 mmHg; all at 37 °C and 1 atm pressure.

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