1. Chapter Six Gas Laws –Properties of Gases –Gas Pressure –Empirical Gas Laws Boyle’s, Charles’ and Gay-Lussac’s –Combined Gas Law –Avogadro’s Law –Dalton’s Law

2. Kinetic Theory of Gases 1.A gas is composed of very small particles. 2.The particles of a gas are very far apart. We assume that the volume of the particles is negligible when compared to the size of the container.

3. Kinetic Theory of Gases 3.Gas particles move very fast in random direction and collide with each other and the walls of the container. An O 2 molecule at 25 o C has an average speed of 1040 mph! pressure is always uniform on any surface of the container.

4. Kinetic Theory of Gases 4.Gas particles do not attract or repel each other. 5.Gas particles move faster, on average, as the temperature increases.

5. Variables Gases are measured in terms of four variables. 1.Pressure (P) – the force exerted by the gas particles –measured in mmHg, atm, torr, and many more. 2.Volume (V) – the space occupied by the gas particles –measured in milliliters or liters

6. Variables 3.Temperature (T) – proportional to the average kinetic energy (speed) of the gas molecules  Celsius or Kelvin (must be used for calculations) 4.Quantity (n) – the amount of gas particles  grams or moles (must be used for calculations)

7. Gas Pressure Gas particles move in random directions and at various speeds.

8. Atmospheric Pressure Atmospheric pressure arises because air particles have mass and are acted upon by the force of gravity. Water exerts a similar, larger force as every 33 feet under water adds an additional force equal to the air.

9. Atmospheric Pressure As altitude increases the pressure ___________. Thus, on top of a mountain, we would see a ______ pressure. And, in Death Valley, which is below sea level, we would see a ______ pressure.

10. Measuring Air Pressure Air pressure is measured with a barometer. At sea level, on an “average” day, the mercury column measures 760 mmHg. This is defined as 1 atmosphere of pressure.

11. Units of Pressure Pressure can be measured in a variety of units.

12. Vapor Pressure If a liquid like water or ethanol is placed in a closed container, some of the liquid particles will evaporate and become gas particles. As temperature increases, so does the vapor pressure.

13. Boiling Point Does water always boil at 100 o C? What would we expect to see in Denver, Colorado? What does a “Pressure Cooker” do?

14. Boling Point and AltitudeAltitude

15. Empirical Gas Laws Allow to examine the relationship between two of the four variables. –Boyle’s Law –Charles’ Law –Gay-Lussac’s Law

16. Boyle’s Law P, V vary while n, T are constant As P , V  and as P , V  When two variables behave this way, we say that they are inversely related. The product of any P and V equals a constant. P * V = constant

17. Boyle’s Law

18. Formula: A 25mL sample of air has a pressure of 750mmHg. If the sample is compressed to 16mL, then what is the pressure of the gas?

19. Charles’ Law V, T vary while n, P are constant As V , T  and as V , T  When two variables behave this way, we say they have a direct or linear relationship Under certain conditions, the ratio of V / T equals a constant.

20. Charles’ Law

21. Formula: A 55mL sample of air in a balloon at 21 o C is warmed to 64 o C. What is the new volume of the balloon?

22. Gay-Lussac’s Law P, T vary while n, V are constant Result is a linear relationship Formula is: A sample of air has a pressure of 0.750atm at 24 o C. If the pressure decreases to 0.552atm, then what is the new temperature (in Celsius)?

23. Combined Gas Law All three gas laws can be combined into one overall formula Once again, Temperatures MUST be in Kelvin

24. Combined Gas Law A 752mL sample of Neon gas has a pressure of 327mmHg at 15 o C. If the pressure is increased to 749mmHg and the temperature is increased to 42 o C, then what is the new volume of the Neon gas?

25. Avogadro’s Law Looks at the relationship between the quantity of gas and its volume The moles of gas are proportional to the volume of that gas

26. STP STP = standard temperature and pressure –Temperature = 0 o C or 273K –Pressure = 760mmHg or 1atm One mole of any gas at STP will occupy 22.4L

27. STP

28. Using STP A reaction produces 0.160g of O 2 at STP. What volume would this occupy? The decomposition of H 2 O 2 generated 152mL of O 2 at STP. What mass of H 2 O 2 reacted? 2 H 2 O 2(aq)  2 H 2 O (l) + O 2(g) What volume of N 2 gas at STP would be generated from the decomposition of 2.50g of NaN 3 ? What volume would it occupy at 22 o C? 2 NaN 3(s)  2 Na (s) + 3 N 2(g)

29. Dalton’s Law For any gas mixture, each gas exerts a pressure proportional to its quantity P total = P A + P B + P C + … P A = P total   A Where

30. Dalton’s Law A gas mixture contains 0.50mol Xe, 0.25mol Kr, and 0.75mol Ar at a total pressure of 3800mmHg. What are the partial pressures of each of the three gases?