1. Characteristic of Gases

2. The Nature of Gases Gases expand to fill their containers Gases are fluid – they flow Gases have low density – 1/1000 the density of the equivalent liquid or solid Gases are compressible Gases effuse and diffuse

3. Gases Are Fluids Gases are considered fluids. The word fluid means “any substance that can flow.” Gas particles can flow because they are relatively far apart and therefore are able to move past each other easily.

4. Gases Have Low Density Gases have much lower densities than liquids and solids do - WHY? – Because of the relatively large distances between gas particles, most of the volume occupied by a gas is empty space. The low density of gases also means that gas particles travel relatively long distances before colliding with each other.

5. Gases are Highly Compressible Suppose you completely fill a syringe with liquid and try to push the plunger in when the opening is plugged. – You cannot make the space the liquid takes up become smaller. The space occupied by the gas particles is very small compared with the total volume of the gas. Applying a small pressure will move the gas particles closer together and will decrease the volume.

6. Gases Completely Fill a Container A solid has a certain shape and volume. A liquid has a certain volume but takes the shape of the lower part of its container. In contrast, a gas completely fills its container. Gas particles are constantly moving at high speeds and are far apart enough that they do not attract each other as much as particles of solids and liquids do. Therefore, a gas expands to fill the entire volume available.

7. Gas Pressure

8. Earth’s atmosphere, commonly known as air, is a mixture of gases: mainly nitrogen and oxygen. As gas molecules are pulled toward the surface of Earth, they collide with each other and with the surface of Earth more often. Collisions of gas molecules are what cause air pressure.

9. Measuring Pressure Pressure = Area Force Newton (N) m 2, cm 2 Units of Pressure 1 atm = 760 torr = 101.3 kPa = 760 mmHg Standard Temperature Pressure (STP) 1 atm, 0°C, 22.4 L, 1 mole

10. 1.00 atm760 mmHg = 7.60 x 10^2 mmHg 1. Covert 1.00 atm to mmHg 1 atm 3.00atm101.3 kPa = 304 kPa 2. Covert 3.00 atm to kPa. 1 atm 3. What is 100.0 KPa in atm? 100.0 kPa 101.3 kPa = 0.9872 atm 1 atm

11. Measures atmospheric pressure The atmosphere exerts pressure on the surface of mercury in the dish. This pressure goes through the fluid and up the column of mercury. The mercury settles at a point where the pressure exerted downward by its weight equals the pressure exerted by the atmosphere. Measuring Pressure Using BarometerBarometer

12. Gas Theory

13. Kinetic Molecular Theory Particles of matter are ALWAYS in motion Volume of individual particles is  zero. Collisions of particles with container walls cause pressure exerted by gas. Particles exert no forces on each other. Average kinetic energy is proportional to Kelvin, temperature of a gas. Ideal gas- imaginary perfect gas fitting the theory

14. Checking for understanding List 5 characteristics of gases: 1. 2. 3. 4. 5. List 5 characteristics of gases according to the KMT: 1. 2. 3. 4. 5.

15. Gas Laws

16. Measurable Properties of Gases Gases are described by their measurable properties. P = pressure exerted by the gas V = total volume occupied by the gas T = temperature of the gas n = number of moles of the gas atm Units L K mol

17. **Gas Laws – ABCGG LAWS** A B C G G vogadro’s oyles’s harles’s ay- Lussac’s n is proportional to V @ constant T P is inversely proportional to V @ constant T V is proportional to T @ constant P P is proportional to T @ constant V raham’s Rate of effusion is inversely proportional to square root of gas’s molar mass

18. Pressure-Volume Relationship : Boyle’s Law Pressure and Volume are inversely proportional at constant temperature  Pressure =  Volume (when one increases the other one decreases)  Volume =  Pressure PV = k P 1 V 1 = P 2 V 2

19. For ALL calculations!!! 1.Circle the numbers, underline what you are looking for. 2.Make a list of number you circled using variables. 3.Write down the formula 4.Derive the formula to isolate the variable you are looking for. 5.Plug in the numbers 6.Answer according to significant figures

20. Boyle’s Law Calculation A given sample of gas occupies 523mL at 1.00 atm. The pressure is increased to 1.97 atm while the temperature stays the same. What is the new volume of the gas? P 1 V 1 = P 2 V 2 P 1 = 1.00 atm P 2 = 1.97 atm V 1 = 523 mLV 2 = ? mL V2=V2= P1V1P1V1 P2P2 = (1.00 atm) (523 mL) (1.97 atm) = 265 mL

21. 1. A sample of oxygen gas has a volume of 150.0mL at a pressure of 0.947 atm. What will the volume of the gas be at a pressure of 1.00 atm if the temperature remains constant? P 1 V 1 = P 2 V 2 P 1 = 0.947 atm P 2 = 1.00 atm V 1 = 150.0 mLV 2 = ? mL V2=V2= P1V1P1V1 P2P2 = (0.947atm) (150.0 mL) (1.00atm) = 142mL

22. 2. If 2.5 L of a gas at 110.0 kPa is expanded to 4.0 L at constant temperature, what will be the new value of pressure? P 1 V 1 = P 2 V 2 P 1 =110.0 kPaP 2 = ? kPa V 1 = 2.5 L V 2 = 4.0 L P2=P2= P1V1P1V1 V2V2 = (110.0 kPa) ( 2.5 L) (4.0 L) = 69 kPa

23. Real World Application BOYLE’S LAW Syringes and turkey basters are operated by Boyle's Law: pulling back on the plunger increases the volume inside the syringe, which decreases the pressure, which then corrects when liquid is drawn into the syringe, thereby shrinking the volume again. Spray cans, like spray paint and air freshener, are governed by Boyle's Law: intense pressure inside the can pushes outward on the liquid inside the can, trying to escape, and forces the liquid out when the cap makes an opening. You breathe because of Boyle's Law. Balloons work because of Boyle's Law. A car (combustion) engine works when the sudden increase in pressure from the combustion of the fuel expands the cylinder and pushes on the piston, causing the crankshaft to turn

24. Temeperature-Volume Relationship: Charle’s Law Volume and temperature are proportional at constant pressure (when gases are heated, they expand)  temperature =  volume (K)  temperature =  Volume (K) = k V T V1V1 T1T1 = V2V2 T2T2  KE of the gases,  volume @  temperature

25. Charles's Law Calculation A balloon is inflated to 665 mL volume at 27°C. It is immersed in a dry-ice bath at −78.5°C. What is its volume, assuming the pressure remains constant? V 1 = 665 mLV 2 = ? mL T 1 = 27 °C + 273 K = 300 K T 2 = -78.5 °C + 273 K = 194.5 K V1V1 T1T1 = V2V2 T2T2 V1V1 T1T1 = V2V2 T2T2 = (665 mL)( 194.5 K) (300 K) = 4.3 x 10^2 mL

26. 1. Helium gas in a balloon occupies 2.5 L at 300.0K. The balloon is dipped into liquid nitrogen that is at a temperature of 80.0K. What will be volume of the helium in the balloon at the lower temperature be? V 1 = 2.5 L T 1 = 300 KT 2 = 80.0 K V1V1 T1T1 = V2V2 T2T2 V1V1 T1T1 = V2V2 = (2.5 L)( 80.0 K) (300 K) = 0.67 L V 2 = ? mL T2T2

27. 2. A helium filled balloon has a volume of 2.75 L at 20.0 °C. The volume of the balloon changes to 2.46 L when placed outside on a cold day. What is the temperature outside in °C ? V 1 = 2.75 L T 1 = 20 °C + 273 K = 293 K T 2 = ? °C V1V1 T1T1 = V2V2 T2T2 V1V1 V2V2 = T2T2 = (2.46 L)( 293 K ) (2.75 L) = 262.10 K = -10.89 °C = -10.9 °C V 2 = 2.46 L T1T1

28. Real World Application CHARLE’S LAW A balloon blown up inside a warm building will shrink when it is carried to a colder area, like the outdoors. Humans' lung capacity is reduced in colder weather; runners and other athletes may find it harder to perform in cold weather for this reason. Charles' Law, along with a couple other gas laws, is responsible for the rising of bread and other baked goods in the oven; tiny pockets of air from yeast or other ingredients are heated and expand, causing the dough to inflate, which ultimately results in a lighter finished baked good. Car (combustion) engines work by this principle; the heat from the combustion of the fuel causes the cylinder to expand, which pushes the piston and turns the crankshaft.

29. Temperature-Pressure Relationships: Gay-Lussac’s Law Pressure and temperature are proportional at constant volume  pressure =  temperature (K)  pressure =  temperature (K) = k P T P1P1 T1T1 = P2P2 T2T2

30. Gay-Lussac’s Law Calculation 1. An aerosol can containing gas at 101 kPa and 22°C is heated to 55°C. Calculate the pressure in the heated can. P 1 = 101 kPa T 1 = 22 °C + 273 K = 295 K T 2 = 55 °C + 273K = 328 K P1P1 T1T1 = P2P2 T2T2 T1T1 P1P1 = P2P2 = (101 kPa)( 328 K ) (295 K) = 110 kPa P 2 = ? kPa T2T2

31. 2. A sample of helium gas is at 122 kPa and 22°C. Assuming constant volume. What will the temperature be when the pressure is 203 kPa? P 1 = 122 kPa T 1 = 22 °C + 273 K = 295 K T 2 = ? K P1P1 T1T1 = P2P2 T2T2 P1P1 P2P2 = T2T2 = (203 kPa)(295K) (122 kPa) = 490K or 220 °C P 2 = 203 kPa T1T1

32. Real World Application GAY-LUSSAC’S LAW Bullets and cannons are based on these principles: gas super- heated by the burning of gun powder is trapped behind the bullet and expands until the bullet leaves the barrel. Someone opening an oven may feel a quick flow of hot air; the air inside the oven is heated, therefore pressurized. The same is true when heating food in closed containers; often, a container will open to release the pressure. If it does not, opening the container will quickly release all the pent-up pressure, which can be very dangerous because the gases inside the hot container may be super-heated. This is why it is always best to open hot containers away from your body and face.

33. Volume-Molar Relationships: Avogadro’s Law Volume and number of moles (n) are proportional at constant temperature and pressure  volume =  number of moles  volume =  number of moles 22.4 L for 1 mole of a gas @ STP = k V n V1V1 n1n1 = V2V2 n2n2

34. Avogadro’s Law What volume of CO 2 contains the same number of molecules as 20.0mL of O 2 at the same conditions? 20 mL

35. Real World Application AVOGADRO’S LAW Avogadro's Law, along with other gas laws, explains why bread and other baked goods rise. Yeast or other leavening agents in the dough break down the long carbohydrates from the flour or sugar and convert them into carbon dioxide gas and ethanol. The carbon dioxide forms bubbles, and, as the yeast continues to leaven the dough, the increase in the number of particles of carbon dioxide increase the volume of the bubbles, thereby puffing up the dough. Avogadro's Law explains projectiles, like cannons and guns; the rapid reaction of the gunpowder very suddenly creates a large amount of gas particles--mostly carbon dioxide and nitrogen gases--which increase the volume of the space behind the cannon or bullet until the projectile has enough speed to leave the barrel. A balloon inflates because of Avogadro's Law; the person blowing into the balloon is inputing a lot of gas particles, so the balloon increases in volume. We breathe because of Avogadro's Law, among others; the lungs expand, so more gas particles can enter the lungs from the outside air (inhaling). Then the lungs contract, so the waste gas particles are expelled (exhaling).

36. Gas Laws Combined Gas Law The ratio of the product of pressure and volume and the temperature of a gas is equal to a constant.pressurevolume temperature

37. Checking for understanding State the law Explain the law in your own words Write the formula(s) Boyle’s Law Charle’s Law Gay-Lussac’s Law Avogadro’s Law

38. Gas Behavior – Diffusion/Effusion Diffusion is the movement of particles from regions of higher density to regions of lower density. Effusion is the passage of gas particles through a small opening is called.

39. Both effusion and difusssion depend on the molar mass of the particle, which determines the speed

40. Effusion

41. Diffusion: describes the mixing of gases. The rate of diffusion is the rate of gas mixing. Molecules move from areas of high concentration to low concentration.

42. Effusion: a gas escapes through a tiny hole in its container -Think of a nail in your car tire… Diffusion and effusion are explained by the next gas law: Graham’s

43. Graham’s Law The rate of effusion and diffusion is inversely proportional to the square root of the molar mass of the molecules. Derived from: Kinetic energy = 1/2 mv 2 m = the molar mass, and v = the velocity. Rate A  Mass B Rate B  Mass A =

44. Sample: compare rates of effusion of Helium with Nitrogen – With effusion and diffusion, the type of particle is important: –Gases of lower molar mass diffuse and effuse faster than gases of higher molar mass. Helium effuses and diffuses faster than nitrogen – thus, helium escapes from a balloon quicker than many other gases! Graham’s Law

45. Big Points to Remember: All gases at the same temperature have the same average kinetic energy. But, they do not have the same average velocity (or speed!) Speed depends on Molar Mass The heavier the gas, the slower it moves! The lighter the gas, the faster it moves!

46. Next slides, not used 2015 Grahams law calculations Dalton’s law Ideal gas law

47. Comparing distance traveled You can compare the distanced traveled by 2 gases in the same amount of time using this equation also. Distance traveled by A =  MassB Distance traveled by B  MassA

48. Graham’s Law The molecular speeds, v A and v B, of gases A and B can be compared according to Graham’s law of diffusion shown below. Graham’s law of diffusion states that the rate of diffusion of a gas is inversely proportional to the square root of the gas’s molar mass. Particles of low molar mass travel faster than heavier particles.

49. Graham’s Law Calculation At the same temperature, which molecule travels faster O 2 or H 2 ? = 3.98 Hydrogen travels 3.98 times faster than oxygen.

50. Graham’s Law Calculation Oxygen molecules have a rate of about 480 m/s at room temperature. At the same temperature, what is the rate of molecules of sulfur hexafluoride, SF 6 ? r O 2 = 480 m/s r SF 6 = ? m/s M O 2 = 32g M SF 6 = 146g = 220 m/s

51. Dalton’s Law The pressure of each gas in a mixture is called the partial pressure. The total pressure of a mixture of gases is the sum of the partial pressures of the gases. This principle is known as Dalton’s law of partial pressure. P total = P A + P B + P C

52. Dalton’s Law Calculation What is the total pressure in a balloon filled with air (O 2 & N 2 ) if the pressure of the oxygen is 170 mm Hg and the pressure of nitrogen is 620 mm Hg? P total = P Oxygen + P nitrogen P total = P A + P B + P C….. = 170 mmHg + 620 mmHg = 790 mmHg

53. Real World Application DALTON’S LAW Dalton's Law is especially important in atmospheric studies. The atmosphere is made up principally of nitrogen, oxygen, carbon dioxide, and water vapors; the total atmospheric pressure is the sum of the partial pressures of each gas. The different partial pressures account for a lot of the weather we experience. Dalton's Law plays a large role in medicine and other breathing areas. Different proportions of gas have different therapeutic effects, so it is important to know the partial pressures of each gas, in a gas line or gas tank, for example.

54. Checking for understanding State the law Explain the law in your own words Write the formula(s) Graham’s Law Dalton’s Law

55. Ideal Gas

56. Molecular Composition of Gases No gas perfectly obeys all four of these laws under all conditions. These assumptions work well for most gases and most conditions. One way to model a gas’s behavior is to assume that the gas is an ideal gas that perfectly follows these laws. An ideal gas, unlike a real gas, does not condense to a liquid at low temperatures, does not have forces of attraction or repulsion between the particles, and is composed of particles that have no volume.

57. Ideal Gas Law PV = nRT P = pressure in atm V = volume in liters n = moles R = proportionality constant – = 0.0821 L atm/ mol·K T = temperature in Kelvins The combined gas law expresses the relationship between pressure, volume and temperature of a fixed amount of gas.

58. Ideal Gas Law Calculation How many moles of gas are contained in 22.4 L liter at 100. atm and 283K? P = 100 atm V = 22.4 L n = ? Moles R = 0.0821 L·atm/mol · K T = 283 K PV = nRT RT PV n = (0.0821 L·atm/mol· K) ( 283 K) (100 atm)(22.4L) = =96.4 moles

59. Calculate the pressure exerted by 43 mol of nitrogen in a 65L of cylinder at 5.0°C. P = ? atmV = 65 L n = 43 mol R = 0.0821 L·atm/mol · K T = 5°C + 273K = 278 K PV = nRT nRT V P = (43 mol)(0.0821 L·atm/mol· K) ( 278 K) (65 L) = =15 atm

60. What will be the volume of 111 mol of nitrogen where the temperature is -57°C and pressure is 250 atm? P = 250 atm V = ? L n = 111 mol R = 0.0821 L·atm/mol · K T = -57°C + 273K = 216 K PV = nRT nRT P V = (111 mol)(0.0821 L·atm/mol· K) ( 216 K) (250 atm) = =7.9 L

61. Real World Application IDEAL GAS LAW The Ideal Gas Law provides important information regarding reactions, like the combination of gases; stoichiometry, like the gas produced in a reaction; physical processes, like the mixing of gases; and thermodynamic processes, like the movement of matter toward disorder. The Ideal Gas Law is used in engineering to determine the capacity of storage containers. It is also helpful in determining the efficiency and standard operation of equipment.

62. Checking for understanding 1.Explain how is ideal gas different from a normal gas. 2. Write the formula for ideal gas 3. What variables can be determined by using the formula?