1. 3 basic gas laws

2. Volume – refers to the space matter (gas) occupies. Measured in liters (L). Pressure – the number of times particles collide with each other and the walls of the container (force exerted on a given area). Measured in atmospheres (atm). 1.000 atm = 760.0 millimeters Hg ( Barometers use Hg) 1.000 atm = 760.0 torr (Named after Torricelli for the invention of the barometer) 1.000 atm = 101.3 kPa – kilopascals Memorize Table 1. P. 542 *all have 4 sig dig STP: standard temperature and pressure (0°C, 101.3 kPa or 1atm). SATP: standard ambient temperature and pressure (25°C, 100 kPa). Definitions

3. Sample Problems Convert 4.400 atm to mmHg. 1 atm=4.40atm 760 mmHg x x = 3344 mmHg Convert 212.4kPa to mmHg. 101.3 kPa=212.4 kPa 760 mmHg x x = 1594 mmHg

4. Temperature – average kinetic energy - as temperate increases gas particles move faster, as temperature decreases gas particles move slower. Measured in Kelvin (K).K = 273 +  C Number of Moles – tells you how much of a certain gas you have 1 mole = number of grams of the compound or element (molar mass) Definitions

5. What is the approximate temperature for absolute zero in degrees Celsius and kelvin? Calculate the missing temperatures 0  C = _______ K100  C = _______ K 100 K = _______  C – 30  C= _______ K 300 K = _______  C 403 K = _______  C 25  C = _______ K0 K = _______  C Kelvin Practice 273373 – 173243 27130 298 – 273 Absolute zero is – 273  C or 0 K

6. Boyle’s Law - Pressure and Volume (when temperature remains constant) V 1 = initial or old volume V 1 P 1 = V 2 P 2 V 2 = final or new volume P 1 = initial or old pressure P 2 = final or new pressure Inverse Relationship (As pressure increases, volume decreases and as pressure decreases, volume increases.)

7. Effect of Pressure on Volume Boyle’s Law 5 1 3 1 atm 1 3 2 atm 5 1 3 5 atm 5

8. Which picture represents what the gas will look like when the pressure is doubled? (Assume constant n, T)

9. P  1/V P x V = constant P 1 x V 1 = P 2 x V 2 5.3 Boyle’s Law Constant temperature Constant amount of gas

10. Kinetic Molecular theory of gases and … Boyle’s Law P  collision rate with wall Collision rate Increases with decreased volume P  1/V Increase P, decrease volume

11. An increase in pressure decreases the volume of air in the lungs.

12. A sample of chlorine gas occupies a volume of 946 mL at a pressure of 726 mmHg. What is the pressure of the gas (in mmHg) if the volume is reduced at constant temperature to 154 mL? P 1 x V 1 = P 2 x V 2 P 1 = 726 mmHg V 1 = 946 mL P 2 = ? V 2 = 154 mL P 2 = P 1 x V 1 V2V2 726 mmHg x 946 mL 154 mL = = 4460 mmHg

13. Sample Problems What is the new pressure when 80.0mL of gas at 500.mmHg is moved to a 100.mL container? (ans: 400. mmHg) A gas at 800.torr of pressure has a volume of 5.00L. What volume does this gas occupy at 1.00X10 3 torr of pressure? (ans: 4.00 L)

14. Charles ’ Law -Volume and Temperature (when pressure is constant) V 1 /T 1 = V 2 /T 2 V 1 = initial or old volume V 2 = final or new volume T 1 = initial or old temperature T 2 = final or new temperature Direct Relationship (As temperature increases, volume increases and as temperature decreases, volume decreases.)

15. The volume of a gas increases with and increase in temperature.

16. If we place a balloon in liquid nitrogen it shrinks: How Volume Varies With Temperature So, gases shrink if cooled. Conversely, if we heat a gas it expands (as in a hot air balloon). Let’s take a closer look at temperature before we try to find the exact relationship of V vs. T.

17. Which picture represents what the gas will look like when the temperature is increased? (Assume constant n, P)

18. Kinetic theory of gases and … Charles’ Law -Average kinetic energy  T -Increase T, Gas Molecules hit walls with greater Force, this Increases the Pressure BUT since pressure must remain constant, and only volume can change -Volume Increase to reduce Pressure -Increase Temperature, Increase Volume

19. A sample of carbon monoxide gas occupies 3.20 L at 125 0 C. At what temperature will the gas occupy a volume of 1.54 L if the pressure remains constant? V 1 = 3.20 L T 1 = 398.15 K V 2 = 1.54 L T 2 = ? T 2 = V 2 x T 1 V1V1 1.54 L x 398.15 K 3.20 L = = 192 K V 1 /T 1 = V 2 /T 2

20. 2.A sample of gas occupies 3.5 L at 300 K. What volume will it occupy at 200 K? 3.If a 1 L balloon is heated from 22°C to 100°C, what will its new volume be? V 1 = 3.5 L, T 1 = 300K, V 2 = ?, T 2 = 200K Using Charles’ law: V 1 /T 1 = V 2 /T 2 3.5 L / 300 K = V 2 / 200 K V 2 = (3.5 L/300 K) x (200 K) = 2.3 L V 1 = 1 L, T 1 = 22°C = 295 K V 2 = ?, T 2 = 100 °C = 373 K V 1 /T 1 = V 2 /T 2, 1 L / 295 K = V 2 / 373 K V 2 = (1 L/295 K) x (373 K) = 1.26 L

21. Gay-Lussac’s Law - Pressure and Temperature (when volume is constant) P 1 /T 1 = P 2 /T 2 P 1 = initial or old pressure P 2 = final or new pressure T 1 = initial or old temperature T 2 = final or new temperature Direct Relationship - As the temperature of the gas increases the pressure of the gas Increases.

22. Sample Problems The gas in an aerosol can is at 3atm of pressure at 298K. What would the gas pressure in the can be at 325K? At 120.  C the pressure of a sample of nitrogen gas is 769torr. What will the pressure be at 205  C?

23. The Combined Gas Law

24. Combining the gas laws So far we have seen three gas laws: Jacques CharlesRobert Boyle P1V1P1V1 =P2V2P2V2 V1V1 T1T1 = V2V2 T2T2 These are all subsets of a more encompassing law: the combined gas law P1P1 T1T1 = P2P2 T2T2 P 1 V 1 P 2 V 2 T 1 T 2 = Joseph Louis Gay-Lussac

25. Sample Problems A helium filled balloon has a volume of 50.0mL at 298K and 1.08atm. What volume will it have at 0.855atm and 203K? Given 700.mL of oxygen at 7.00  C and 7.90atm of pressure, what volume does is occupy at 27.0  C and 4.90atm of pressure? Note: any unit for pressure will work, provided the same units are used throughout. The only unit that MUST be used is K for temperature.

26. CW/ HW Complete ISU booklet – 1 st page Practice questions on 1 st 3 laws on 2 nd page