1. Chemistry 14.4

2. Gases: Mixtures and Movements
A list of gear for an expedition to Mount Everest includes climbing equipment, ski goggles, a down parka with a hood, and most importantly compressed-gas cylinders of oxygen. You will find out why a supply of oxygen is essential at higher altitudes.

3. Dalton’s Law
Dalton’s Law
How is the total pressure of a mixture of gases related to the partial pressures of the component gases?

4. Dalton’s Law
The contribution each gas in a mixture makes to the total pressure is called the partial pressure exerted by that gas.

5. Dalton’s Law
In a mixture of gases, the total pressure is the sum of the partial pressures of the gases.

6. Dalton’s Law
Dalton’s law of partial pressures states that, at constant volume and temperature, the total pressure exerted by a mixture of gases is equal to the sum of the partial pressures of the component gases.

7. Observe the behavior of a mixture of nonreacting gases.
Dalton’s Law
Animation 17
Observe the behavior of a mixture of nonreacting gases.

8. Three gases are combined in container T.
Dalton’s Law
Three gases are combined in container T.
Three gases are combined in container T. The pressure that each gas exerts is independent of the pressure exerted by the other two gases. The pressure in container T is the sum of the pressures in containers A, B, and C. Interpreting Diagrams What is the relationship between the number of particles in containers A and C and the partial pressures of the gases in A and C?

9. Dalton’s Law
The partial pressure of oxygen must be kPa or higher to support respiration in humans. The climber below needs an oxygen mask and a cylinder of compressed oxygen to survive.
This climber is using a tank of compressed gas to supplement the supply of oxygen available at high altitudes.

10. 14.6
Firefighters carry tanks of compressed air. The tanks contain from 19.5% to 23.5% oxygen by volume.

11. 14.6

12. 14.6

13. 14.6

14. Solve Problem 32 with the help of an interactive guided tutorial.
for Sample Problem 14.6
Problem Solving 14.32
Solve Problem 32 with the help of an interactive guided tutorial.

15. Graham’s Law
Graham’s Law
How does the molar mass of a gas affect the rate at which the gas effuses or diffuses?

16. Graham’s Law
Diffusion is the tendency of molecules to move toward areas of lower concentration until the concentration is uniform throughout.

17. Graham’s Law
Bromine vapor is diffusing upward through the air in a graduated cylinder.
The diffusion of one substance through another is a relatively slow process. a) Bromine vapor is diffusing upward through the air in a graduated cylinder. b) After several hours, bromine vapors are near the top of the cylinder. Predicting What will happen as the bromine continues to diffuse?

18. Graham’s Law
After several hours, the bromine has diffused almost to the top of the cylinder.
The diffusion of one substance through another is a relatively slow process. a) Bromine vapor is diffusing upward through the air in a graduated cylinder. b) After several hours, bromine vapors are near the top of the cylinder. Predicting What will happen as the bromine continues to diffuse?

19. During effusion, a gas escapes through a tiny hole in its container.
Graham’s Law
During effusion, a gas escapes through a tiny hole in its container.
Gases of lower molar mass diffuse and effuse faster than gases of higher molar mass.

20. Thomas Graham’s Contribution
Graham’s Law
Thomas Graham’s Contribution
Graham’s law of effusion states that the rate of effusion of a gas is inversely proportional to the square root of the gas’s molar mass. This law can also be applied to the diffusion of gases.

21. Comparing Effusion Rates
Graham’s Law
Comparing Effusion Rates
A helium filled balloon will deflate sooner than an air-filled balloon.
The character balloons used in parades are filled with helium gas so that they will float.

22. Graham’s Law
Helium atoms are less massive than oxygen or nitrogen molecules. So the molecules in air move more slowly than helium atoms with the same kinetic energy.

23. Graham’s Law
Because the rate of effusion is related only to a particle’s speed, Graham’s law can be written as follows for two gases, A and B.

24. Graham’s Law
Helium effuses (and diffuses) nearly three times faster than nitrogen at the same temperature.

25. Observe the processes of gas effusion and diffusion.
Graham’s Law
Animation 18
Observe the processes of gas effusion and diffusion.

26. 14.4 Section Quiz.
14.4.

27. 14.4 Section Quiz.
1. What is the partial pressure of oxygen in a diving tank containing oxygen and helium if the total pressure is 800 kPa and the partial pressure of helium is 600 kPa?
200 kPa
0.75 kPa
kPa
1.33 kPa

28. 14.4 Section Quiz.
2. A mixture of three gases exerts a pressure of 448 kPa, and the gases are present in the mole ratio 1 : 2 : 5. What are the individual gas pressures?
44 kPa, 88 kPa, and 316 kPa
52 kPa, 104 kPa, and 292 kPa
56 kPa, 112 kPa, and 280 kPa
84 kPa, 168 kPa, and 196 kPa

29. 14.4 Section Quiz.
3. Choose the correct words for the spaces. Graham's Law says that the rate of diffusion of a gas is __________ proportional to the square root of its _________ mass.
directly, atomic
inversely, atomic
inversely, molar
directly, molar

30. Solve the Concept Map with the help of an interactive guided tutorial.

31. END OF SHOW