1. CATALYST: PICK UP PAPERS IN THE FRONT WRITE OUT THE SOLUBILITY RULES!

2. CATALYST: PICK UP PAPERS IN THE FRONT WRITE AN EQUATION TO FIND THE MOLAR MASS USING THE IDEAL GAS LAW

3. Explosion Questions 1.What is the law of conservation of mass? 2.What is the law of definite proportions? 3.What is the law of multiple proportions? 4.Who discovered the electron? 5.Who is Ernest Rutherford? 6.How do you find the number of neutrons? 7.What is an isotope? 8.What is the formula for Nitrite? 9.What is the formula for Perchlorate? 10.What is the formula for Hyposulfite? 11.What is the empirical formula? 12.What is the molecular formula? 13.What is the limiting reagent? 14.What is the % yield? 15.What is % composition? 16.Name the strong acids 17.Name the Strong bases 18.Is Lead Nitrate Soluble? 19.Is Mercury Sulfate soluble? 20.All halogens are soluble except what? 21.What is an Ideal Gas? 22.What is Boyle’s law between? 23.What is Charles Law between? 24.What is Avogadro’s law between? 25.What is the combined gas law?

4. LAB

5. UNIT 2: CH. 5 GASES!

6. GAS STOICHIOMETRY

7. DALTON’S LAW OF PARTIAL PRESSURE P total = P 1 + P 2 + P 3 + … The total pressure of a gas is the sum of the pressures that each gas would exert alone Partial Pressure - P 1, P 2, P 3

8. DALTON’S LAW OF PARTIAL PRESSURE P total = P 1 + P 2 + P 3 + … Example: Mixtures of He and Oxygen can be used in scuba diving tanks to help prevent “the bends.” For a particular dive, 46 L He at 25 °C and 1.0 atm and 12 L oxygen at 25 °C and 1.0 atm were pumped into a tank with a volume 5.0 L/ calculate the partial pressure of each gas and the total pressure in the tank at 25 °C

9. ASSUMING AN IDEAL GAS… Derive how Dalton’s Law of Partial Pressure and Ideal Gas Law can be combined. Pressure of an ideal gas is not affected by the identity of the gas: (1)Volume of the individual gas is not important (2)Forces among particles must not be important

10. ASSUMING AN IDEAL GAS… Derive how Dalton’s Law of Partial Pressure and Ideal Gas Law can be combined.

11. MOLE FRACTION The ratio of the number of moles of a given component in a mixture to the total number of moles in the mixture:

12. MOLE FRACTION Example: The mole fraction of nitrogen in the air is 0.7808. Calculate the partial Pressure of Nitrogen in air when the atmospheric pressure is 760 torr.

13. VAPOR PRESSURE OF WATER When the rate of water evaporation = rate of condensation, the number of molecules in the vapor state remains constant as well as the pressure. Example: A sample of solid Potassium Chlorate was heated in a test tube and decomposed. The oxygen produced was colleved by displacement of water at 22 °C at a total pressure of 754 torr. The volume of gas collected was 0.650 L and the vapor pressure of water at 22 °C is 21 torr. Calculate the Partial Pressure of oxygen in the gas collected and the mass of potassium chlorate that was decomposed.

14. PRACTICE TIME!

15. CATALYST: PICK UP PAPERS IN THE FRONT Calculate the density of Ammonia at STP

16. Explosion Questions 1.What is the law of conservation of mass? 2.What is the law of definite proportions? 3.What is the law of multiple proportions? 4.Who discovered the electron? 5.Who is Ernest Rutherford? 6.How do you find the number of neutrons? 7.What is an isotope? 8.What is the formula for Nitrite? 9.What is the formula for Perchlorate? 10.What is the formula for Hyposulfite? 11.What is the empirical formula? 12.What is the molecular formula? 13.What is the limiting reagent? 14.What is the % yield? 15.What is % composition? 16.Name the strong acids 17.Name the Strong bases 18.Is Lead Nitrate Soluble? 19.Is Mercury Sulfate soluble? 20.All halogens are soluble except what? 21.What is an Ideal Gas? 22.What is Boyle’s law between? 23.What is Charles Law between? 24.What is Avogadro’s law between? 25.What is the combined gas law?

17. UNIT 2: CH. 5 GASES!

18. KMT

19. KINETIC MOLECULAR THEORY OF GASES! This is a MODEL! Which is successful if it explains the observed behavior and predicts the results of future experiments KMT explains ideal gases, real gases have volume so they do not fit correctly

20. KINETIC MOLECULAR THEORY OF GASES! The volume of an individual particles is assumes negligible (can be ignored) Particles are in constant motion and the collisions of the particles with the walls of the container are what causes the pressure exerted by the gas Particles are assumed to neither attract nor repel each other (no forces between each other) The average kinetic energy (amount of movement) of gas particles is directly proportional to the temperature (K) of the gas

21. LET’S CHECK! Pressure and Volume (Boyle’s Law): follows KMT: decrease in V  more collisions with the walls  increase in P Pressure and Temperature: follows KMT: temp increases  speed of particles increase  so hit wall with more force and more times  increase in P Volume and Temperature (Charles’s Law): follows KMT: temp increase  speed of molecules increase  if P is constant, only way to compensate for increased speed is to increase volume Volume and Number of Moles (Avogadro’s Law): Follows KMT: more molecules at constant temp  to return P to original constant  increase V Mixture of Gases (Dalton’s Law): Follows KMT: total P is the sum of partial pressures follows KMT  no forces assumed between particles and volumes of particles are unimportant

22. DERIVING THE IDEAL GAS LAW FROM PRESSURE! Pressure Eqn from Appendix B Where the average kinetic energy equals… Finish on Board! N A = Avogadro’s number m = mass (kg) u 2 = average velocity squared N = # of moles

23. MEANING OF TEMPERATURE Kinetic Energy into the pressure equation…let’s derive the relationship between KE and Temperature!

24. ROOT MEAN SQUARE VELOCITY Average particle velocity (u rms ) We can solve for RMS velocity using Kinetic Energy!

25. EFFUSION AND DIFFUSION

26. DIFFUSION Diffusion – describes the mixing of gases Ex. The time it takes for a gas to mix in air

27. EFFUSION Effusion – the speed at which a gas to passes through a tiny hole/membrane into an evacuated (completely empty) chamber

28. GRAHAM’S LAW OF EFFUSION M 1 = molar mass of gas 1 M 2 = molar mass of gas 2 Derive from u rms Where M = kg/mol

29. EXAMPLE PROBLEM Calculate the ratio of the effusion rates of hydrogen gas and uranium hexafluoride, a gas used in the enrichment process to produce fuel for nuclear reactors.

30. PRACTICE PROBLEMS!