Presentation is loading. Please wait.

Presentation is loading. Please wait.

Physical Characteristics of Gases Chapter 10. 2 Kinetic-molecular theory Particles of matter are always in motion Chemistry Chapter 10.

Similar presentations


Presentation on theme: "Physical Characteristics of Gases Chapter 10. 2 Kinetic-molecular theory Particles of matter are always in motion Chemistry Chapter 10."— Presentation transcript:

1 Physical Characteristics of Gases Chapter 10

2 2 Kinetic-molecular theory Particles of matter are always in motion Chemistry Chapter 10

3 3 Ideal gas An imaginary gas that perfectly fits all the assumptions of the kinetic- molecular theory. We can often treat real gases as ideal gases and still get good results. Chemistry Chapter 10

4 4 Assumptions of KMT of gases 1.Large numbers of tiny particles that are far apart compared to their size Low density Easily compressed 2.Elastic collisions No kinetic energy is lost when gas particles collide with each other or their container It can be transferred between particles, but the total kinetic energy remains the same Chemistry Chapter 10

5 5 3.Gas particles are in continuous, rapid, random motion 4.There are no attractive or repulsive forces between gas particles When they hit, they don’t stick together 5.The average kinetic energy of gas particles depends on the temperature of the gas Direct relationship Chemistry Chapter 10

6 6 Expansion Gases have indefinite shape and volume. They completely fill any container they are in. They also take the shape of that container. Because: –they move rapidly in all directions and don’t stick together Chemistry Chapter 10

7 7 Fluidity Gas particles slide past each other. They can flow –Fluid: something that can flow (can be gas or liquid) Chemistry Chapter 10

8 8 Diffusion Spontaneous mixing of the particles of two substances caused by their random motion. Gas particles spread out to fill their new container Chemistry Chapter 10

9 9 Effusion When gas particles pass through a small opening Particles leak out of the container Chemistry Chapter 10

10 10 Real gases Do not completely follow kinetic- molecular theory Especially deviant at high pressures and low temperatures Noble gases are closest to ideal Very polar gases are farthest from ideal Chemistry Chapter 10

11 11 Discuss Describe the conditions under which a real gas is most likely to behave ideally. Explain the following properties of gases using the kinetic-molecular theory: expansion, fluidity, low density, compressibility, and diffusion. Chemistry Chapter 10

12 12 Describing gases Needed: –Volume –Temperature –Number of molecules –Pressure They are mathematically related. Chemistry Chapter 10

13 13 Pressure balloon The force per unit area on a surface. Chemistry Chapter 10

14 14 Force A push or a pull Measured in newtons (N). At the Earth’s surface, 1 kg of mass exerts 9.8 N of force due to gravity. Chemistry Chapter 10

15 15 Chemistry Chapter 10

16 16 Pressure of gases Gases exert pressure on any surface with which they collide. –Depends on volume, temperature, and number of molecules Chemistry Chapter 10

17 17 Atmospheric pressure Air around Earth exerts a pressure on it’s surface and everything on it. –Like the weight of all the molecules pressing down. Chemistry Chapter 10

18 18 Barometer Used to measure atmospheric pressure. Height of liquid (usually mercury) in tube can be used to express atmospheric pressure. At sea level, the average is 760 mm Hg. h Chemistry Chapter 10

19 19 Manometer Used to measure the pressure of gases. The height difference between the two arms is the pressure. Chemistry Chapter 10

20 20 Pressure Units Chemistry Chapter 10

21 21 STP Standard temperature and pressure. 0 °C and 1 atm Used to compare volumes of gases. Chemistry Chapter 10

22 22 Example A weather report gives a current atmospheric pressure of mm Hg. Convert this to –Atmospheres atm –Torr torr –Kilopascals kPa Chemistry Chapter 10

23 23 Discuss Define pressure What is STP? Convert kPa to atmospheres – atm Chemistry Chapter 10

24 24 Boyle’s Law Fixed: mass and temperature The volume varies inversely with pressure –Less volume, means the particles hit the walls more often. –This increases the pressure Chemistry Chapter 10

25 25 Boyle’s Law Mathematically: Each sample of gas has its own k. Chemistry Chapter 10

26 26 Example A helium-filled balloon contains 125 mL of gas at a pressure of atm. What volume will the gas occupy at standard pressure, assuming constant temperature? 122 mL Chemistry Chapter 10

27 27 You try A weather balloon with a volume of L is released from Earth’s surface at sea level. What volume will the balloon occupy at an altitude of 20.0 km, where the air pressure is 10.0 kPa, assuming constant temperature? 13.9 L Chemistry Chapter 10

28 28 Charles’s Law Fixed: mass and pressure Volume varies directly with temperature. –As temperature goes up, the particles have more energy, so they hit the walls more often and with more force –This pushes the walls outward. Chemistry Chapter 10

29 29 Charles’s Law Mathematically Chemistry Chapter 10

30 30 Kelvin Scale Charles’s law works more elegantly on the Kelvin Scale than the Celsius Scale. –If you double the temperature, the volume doubles. Not true with Celsius We must use Kelvin for Charles’s Law. Chemistry Chapter 10

31 31 Kelvin Scale Absolute zero: lowest possible temperature –All particle motion stops –0 K, °C Often rounded to 273 Chemistry Chapter 10

32 32 Example A balloon filled with oxygen gas occupies a volume of 5.5 L at 25 °C. What volume will the gas occupy at 100. °C, assuming constant pressure? 6.9 L Chemistry Chapter 10

33 33 You try A sample of nitrogen gas is contained in a piston with a freely moving cylinder. At 0.0 °C, the volume of the gas is 375 mL. To what temperature must the gas be heated to occupy a volume of 500. mL, assuming constant pressure? 91 °C Chemistry Chapter 10

34 34 Gay-Lussac’s Law Fixed: mass and volume Pressure varies directly with temperature (in Kelvin) –As temperature goes up, energy of particles goes up. –They go faster and hit the walls harder. –If the walls can’t move, the pressure goes up. Chemistry Chapter 10

35 35 Gay-Lussac’s Law Mathematically: Chemistry Chapter 10

36 36 You try The temperature within an automobile tire at the beginning of a long trip is 25 °C. At the conclusion of the trip, the tire has a pressure of 1.80 atm. What is the final Celsius temperature within the tire if its original pressure was 1.75 atm? Assume constant volume. 34 °C Chemistry Chapter 10

37 37 Combined gas law Expresses the relationship between pressure, volume, and temperature of a fixed amount of gas. Chemistry Chapter 10

38 38 You try The volume of a gas at 27.0 °C and atm is 80.0 mL. What volume will the same gas sample occupy at standard conditions? 14.6 mL Chemistry Chapter 10

39 39 Dalton’s Law The total pressure in a container is the sum of the partial pressures of all the gases in the container. Chemistry Chapter 10

40 40 Application We can collect gases by displacing water. When we do this, Read P atm from the barometer. Look up P water in table A-8 in the appendix. Chemistry Chapter 10

41 41 Example A student has stored mL of neon gas over water on a day when the temperature is 27.0 °C. If the barometer in the room reads mm Hg, what is the pressure of the neon gas in its container? mm Hg Chemistry Chapter 10

42 42 You try A sample of nitrogen gas is collected over water at a temperature of 23.0 °C. What is the pressure of the nitrogen gas if atmospheric pressure is 785 mm Hg? 764 mm Hg Chemistry Chapter 10


Download ppt "Physical Characteristics of Gases Chapter 10. 2 Kinetic-molecular theory Particles of matter are always in motion Chemistry Chapter 10."

Similar presentations


Ads by Google