1. Chapter 13: Gases

2. What Are Gases? Gases have mass Gases have mass

3. Properties of Gases Easy to compress Easy to compress

4. What Are Gases? Fill their containers completely Fill their containers completely

5. What Are Gases? Move very quickly Move very quickly Movement of gases is called diffusion Movement of gases is called diffusion

6. What Are Gases? Gases exert pressure Gases exert pressure Pressure is due to collisions Pressure is due to collisions

7. Describing Behavior of Gases Depends upon 4 variables Depends upon 4 variables 1. Amount of Gas (n) – Measured in Moles (mol) 2. Volume (V) – Measure in Liters (L) 3. Temperature (T) – Measured in Kelvin (K) 4. Pressure (P) – Measured in Pascals (Pa)

8. Pressure Pressure is the amount of force per given area Pressure is the amount of force per given area One newton of force per square meter is the Pascal One newton of force per square meter is the Pascal Often measure in kPa Often measure in kPa 1013.25 millibars (mb) = 101.325 kPa = 1 atmosphere (atm) = 14.7 pounds per in 2 (psi) = 760 mm of Hg (torr) 1013.25 millibars (mb) = 101.325 kPa = 1 atmosphere (atm) = 14.7 pounds per in 2 (psi) = 760 mm of Hg (torr)

9. Atmospheric Pressure Pressure exerted by the atmosphere Pressure exerted by the atmosphere

10. Atmospheric Pressure Air Pressure measured by a barometer Air Pressure measured by a barometer Measured in mmHg Measured in mmHg

11. Practice High Pressure 1085 mb in Mongolia (2001) Convert to kPa High Pressure 1085 mb in Mongolia (2001) Convert to kPa Low Pressure 870 mb in a Pacific Typhoon (1979) Convert to Atm Low Pressure 870 mb in a Pacific Typhoon (1979) Convert to Atm

12. Kinetic Molecular Theory The behavior of gas is explained by the K–M theory of matter The behavior of gas is explained by the K–M theory of matter 1. Gases consist of particles that have mass 2. There are large distances between gas particles 3. Gas particles are in constant random motion

13. Kinetic Molecular Theory 4. Collisions of gas particles with other particles or with the walls of the container are completely elastic. Elastic collision

14. Kinetic Molecular Theory 5. Kinetic energy of gas depends upon temperature –High temperature, high KE 6. Gas particles exert no attractive forces between one another www.falstad.com/gas/

15. Boyle’s Law The pressure and volume of a sample of gas are inversely proportional at constant temperature The pressure and volume of a sample of gas are inversely proportional at constant temperature “spring of air” “spring of air” P 1 V 1 =P 2 V 2 P 1 V 1 =P 2 V 2

17. Charles’s Law At constant pressure, the volume of a fixed amount of gas is directly proportional to its temperature. At constant pressure, the volume of a fixed amount of gas is directly proportional to its temperature. Helped determine absolute zero Helped determine absolute zero V 1 /T 1 =V 2 /T 2 V 1 /T 1 =V 2 /T 2 All temperatures must be converted to Kelvin All temperatures must be converted to Kelvin

20. Practice A weather balloon contains 150. L of gas, internal gas pressure is 1.0 atm. Atmospheric pressure at 41 km is 0.4 atm. Calculate the new volume of the balloon. A weather balloon contains 150. L of gas, internal gas pressure is 1.0 atm. Atmospheric pressure at 41 km is 0.4 atm. Calculate the new volume of the balloon. A sample of gas has a volume of 1 L at -18 0 C. What is the temperature if the volume of the same gas is changed to 0.45 Liters? A sample of gas has a volume of 1 L at -18 0 C. What is the temperature if the volume of the same gas is changed to 0.45 Liters?

21. Practice What will be the volume of a gas sample at 355 K if its volume at 273 K is 8.57 Liters? What will be the volume of a gas sample at 355 K if its volume at 273 K is 8.57 Liters? 2.00 L of a gas is at 740.0 mmHg pressure. What is its volume at standard pressure? 2.00 L of a gas is at 740.0 mmHg pressure. What is its volume at standard pressure?

22. Dalton’s Law Dalton’s Law of Partial Pressure states that the sum of the partial pressures of all of the components in a gas mixture is equal to the total pressure of the gas mixture. Dalton’s Law of Partial Pressure states that the sum of the partial pressures of all of the components in a gas mixture is equal to the total pressure of the gas mixture. P T = P a + P b + P c …. P T = P a + P b + P c ….

24. Combined Gas Law We can take all of the pressure- volume-temperature relationships we’ve just talked about and combine them into one gas law: (P 1 V 1 )/T 1 = (P 2 V 2 )/T 2 If you remember this gas law, you can figure out the others.

25. Practice What is atmospheric pressure if the partial pressures of N 2, O 2, and Ar are 604.5 mm Hg, 162.8 mm Hg, and 0.5 mm Hg respectively? What is atmospheric pressure if the partial pressures of N 2, O 2, and Ar are 604.5 mm Hg, 162.8 mm Hg, and 0.5 mm Hg respectively? If I have 21 liters of gas held at a pressure of 78 atm and a temperature of 900. K, what will be the volume of the gas if I decrease the pressure to 45 atm and decrease the temperature to 750 K?

26. Ideal Gas Law The ideal gas law combines all variables involved in a gas. The ideal gas law combines all variables involved in a gas. PV = nRT R is a constant R is a constant R = 0.0821 atm-L/mol-K R = 0.0821 atm-L/mol-K Temp must be in K Temp must be in K Pressure must be in Atm Pressure must be in Atm Volume must be in Liters Volume must be in Liters

27. Ideal Gas vs. Real Gas An Ideal Gas represents a gas as described by the kinetic-molecular theory. An Ideal Gas represents a gas as described by the kinetic-molecular theory. Assumes no interaction between gas molecules Assumes no interaction between gas molecules All gases are Real Gas All gases are Real Gas An ideal gas behaves >95% like a real gas. An ideal gas behaves >95% like a real gas. Real Gases deviate from ideal gases at low temperatures and high pressures. Real Gases deviate from ideal gases at low temperatures and high pressures.

28. Practice How many moles of a gas at 100. o C does it take to fill a 1.00 Liter flask to a pressure of 1.50 atm? How many moles of a gas at 100. o C does it take to fill a 1.00 Liter flask to a pressure of 1.50 atm? What is the volume occupied by 9.45 g of C 2 H 2 at STP? What is the volume occupied by 9.45 g of C 2 H 2 at STP?

29. Atmospheric Pressure Air pressure changes with altitude Air pressure changes with altitude

30. Atmospheric Pressure Air pressure changes due to the heating by the sun Air pressure changes due to the heating by the sun

31. Manometer Enclosed gases may be measured by a manometer Enclosed gases may be measured by a manometer Pressure of gas = height + air pressure Pressure of gas = height + air pressure

32. Guy Lussac’s Law At constant volume, the pressure of a fixed amount of gas is directly proportional to its temperature. At constant volume, the pressure of a fixed amount of gas is directly proportional to its temperature. P 1 /T 1 =P 2 /T 2 P 1 /T 1 =P 2 /T 2 All temperatures must be converted to Kelvin All temperatures must be converted to Kelvin Autoclaves Autoclaves

33. Practice You fill your car tires to 35 psi in the summer when it’s 31 °C. At Thanksgiving, when it’s -7 °C, you notice that your tire is low. What is the pressure inside your tires?

34. Avogadro's Law Avogadro’s Law states equal volumes of gases at the same temperature and pressure contain an equal number of particles. Avogadro’s Law states equal volumes of gases at the same temperature and pressure contain an equal number of particles. Volume and amount are directly proportional. Volume and amount are directly proportional. V 1 /n 1 = V 2 /n 2 V 1 /n 1 = V 2 /n 2

35. Practice The gases of carbon dioxide, oxygen, nitrogen, neon, and krypton are mixed in a container. All gases have the same partial pressure and the total pressure is 33,500 Pa. What is the partial pressure of nitrogen? The gases of carbon dioxide, oxygen, nitrogen, neon, and krypton are mixed in a container. All gases have the same partial pressure and the total pressure is 33,500 Pa. What is the partial pressure of nitrogen?

36. Practice I have an unknown volume of gas at a pressure of 0.5 atm and a temperature of 325 K. If I raise the pressure to 1.2 atm, decrease the temperature to 320 K, and measure the final volume to be 48 liters, what was the initial volume of the gas? If I have 21 liters of gas held at a pressure of 78 atm and a temperature of 900 K, what will be the volume of the gas if I decrease the pressure to 45 atm and decrease the temperature to 750 K?