2. TUTORIAL INSTRUCTIONS: Carefully go through the tutorial, step by step. You may return to any section, as necessary. Once you are satisfied that you understand the concepts and procedures, click CLOSE to get out of the tutorial mode. You will then be taken to the post-quiz. PLEASE LISTEN CAREFULLY CLICK TO CONTINUE

3. doubling the number of particles doubles the amount of gas in the sample and halving the number of particles halves the amount of gas that is present in the sample. LISTEN THOUGHTFULLY GO AT YOUR OWN PACE MAKE NOTES AS NECESSARY (MEASURING GASSES) CLICK TO CONTINUE

4. Pressure is the force with which the gas particles bombard one unit of surface area of the container. LISTEN THOUGHTFULLY GO AT YOUR OWN PACE MAKE NOTES AS NECESSARY (MEASURING GASSES) CLICK TO CONTINUE

5. At higher temperatures the average energy of the gas particles is greater and at lower temperatures the average energy of the gas particles is less. LISTEN THOUGHTFULLY GO AT YOUR OWN PACE MAKE NOTES AS NECESSARY (MEASURING GASSES) CLICK TO CONTINUE

6. The volume of a gas is the volume of the container. LISTEN THOUGHTFULLY GO AT YOUR OWN PACE MAKE NOTES AS NECESSARY (MEASURING GASSES) CLICK TO CONTINUE

7. IDEAL GAS LAW PV = nRT LISTEN THOUGHTFULLY GO AT YOUR OWN PACE MAKE NOTES AS NECESSARY (RELATING GAS PROPERTIES) CLICK TO CONTINUE

8. When the units of pressure and volume are, respectively, atmosphere and liter, R has a value of 0.082053 L atm. mol K LISTEN THOUGHTFULLY GO AT YOUR OWN PACE MAKE NOTES AS NECESSARY (RELATING GAS PROPERTIES)

9. When the units of pressure and volume are, respectively, torr and milliliter, R has a value of 62360.3 mL torr. mol K (RELATING GAS PROPERTIES)

10. When the units of pressure and volume are, respectively, pascal and meters cubed R has a value of 8.3144 pa m 3. mol K CLICK TO CONTINUE (RELATING GAS PROPERTIES)

11. R = PV nT LISTEN THOUGHTFULLY GO AT YOUR OWN PACE MAKE NOTES AS NECESSARY (RELATING GAS PROPERTIES) CLICK TO CONTINUE

12. an increase in the gas pressure decreases the volume, and a decrease in gas pressure increases volume. This is called Boyle’s Law. LISTEN THOUGHTFULLY GO AT YOUR OWN PACE MAKE NOTES AS NECESSARY (RELATING PRESSURE, VOLUME) CLICK TO CONTINUE

13. an increase in the amount of gas is accompanied by a decrease in temperature, and a decrease in the amount of gas is accom- panied by an increase temperature. LISTEN THOUGHTFULLY GO AT YOUR OWN PACE MAKE NOTES AS NECESSARY (RELATING AMOUNT, TEMPERATURE) CLICK TO CONTINUE

14. a larger gas sample will exert more pressure, a smaller gas sample will exert less pressure. LISTEN THOUGHTFULLY GO AT YOUR OWN PACE MAKE NOTES AS NECESSARY (RELATING AMOUNT, PRESSURE) CLICK TO CONTINUE

15. And so, a gas sample that is composed of CO(g) at two atmospheres, Ar(g) at three atmospheres and O 2 (g) at one atmosphere will have a total pressure of six atmospheres. LISTEN THOUGHTFULLY GO AT YOUR OWN PACE MAKE NOTES AS NECESSARY (PRESSURE OF GASEOUS MIXTURE) CLICK TO CONTINUE

16. Dalton’s Law of Partial Pressures states that the total pressure of a mixture of gases is the sum of the partial pressures of the gasses in the mixture. LISTEN THOUGHTFULLY GO AT YOUR OWN PACE MAKE NOTES AS NECESSARY (PRESSURE OF GASEOUS MIXTURE) CLICK TO CONTINUE

17. a bigger volume of gas will have a higher temperature and a smaller volume of gas will have a lower tempera- ture. This is Charles’ Law. LISTEN THOUGHTFULLY GO AT YOUR OWN PACE MAKE NOTES AS NECESSARY (RELATING VOLUME, TEMPERATURE) CLICK TO CONTINUE

18. a larger gas sample will occupy a larger volume, and a smaller gas sample will occupy a smaller volume. This is Avagadro’s Law. LISTEN THOUGHTFULLY GO AT YOUR OWN PACE MAKE NOTES AS NECESSARY (RELATING VOLUME, AMOUNT) CLICK TO CONTINUE

19. an increase in temperature is accompanied by an increase in gas pressure and a decrease in the temperature is accompanied by a decreases in gas pressure. This is Gay-Lussac’s Law. LISTEN THOUGHTFULLY GO AT YOUR OWN PACE MAKE NOTES AS NECESSARY (RELATING PRESSURE, TEMPERATURE) CLICK TO CONTINUE

20. P 1 V 1 = P 2 V 2 T 1 T 2 COMBINED GAS LAW: LISTEN THOUGHTFULLY GO AT YOUR OWN PACE MAKE NOTES AS NECESSARY (RELATING PRESSURE, VOLUME, TEMPERATURE) CLICK TO CONTINUE

21. Example 1: A student prepares chlorine gas in the chemistry lab where the temperature is 20 o C, and collects it in a gas jar over water. On that day the atmospheric pressure is 0.997 atm. At 20 o C water has a vapor pressure of 17.5 torrs. What was the actual press- ure of the chlorine collected? CLICK TO CONTINUE LISTEN THOUGHTFULLY GO AT YOUR OWN PACE MAKE NOTES AS NECESSARY (GAS LAW CALCULATION)

22. The properties given are temperature (20 0 C), atmospheric pressure (0.997 atm), water vapor pressure at 20 0 (17.5 torr). The property to be found is pressure of chlorine gas. LISTEN THOUGHTFULLY GO AT YOUR OWN PACE MAKE NOTES AS NECESSARY (ANALYSIS OF THE PROBLEM)

23. P tot = P atm = P chlorine + P water vapor LISTEN THOUGHTFULLY GO AT YOUR OWN PACE MAKE NOTES AS NECESSARY (FORMATING THE SOLUTION) CLICK TO CONTINUE 0.997 atm P chlorine = 0.997 atm - 17.5 torr P tot = P 1 + P 2 + P 3 +… = P chlorine + 17.5 torr

24. CLICK TO CONTINUE = 0.997 atm - 17.5 torr P tot = P atm = P chlorine + P water vapor P tot = P 1 + P 2 + P 3 +… LISTEN THOUGHTFULLY GO AT YOUR OWN PACE MAKE NOTES AS NECESSARY (FORMATING THE SOLUTION) = P atm - P water vapor P chlorine

25. 0.997 atm x 760 torrs 1 atm = 758 torrs P chlorine = 758 torrs – 17.5 torrs = 740 torrs CLICK TO CONTINUE LISTEN THOUGHTFULLY GO AT YOUR OWN PACE MAKE NOTES AS NECESSARY (UNIT CONVERSION, EVALUATION)

26. LISTEN THOUGHTFULLY GO AT YOUR OWN PACE MAKE NOTES AS NECESSARY (GAS LAW CALCULATION) CLICK TO CONTINUE Example 2: A sample of neon which occupies 40 mL at 800 torrs and 30 o C is transferred to another container in which it attains S.T.P. conditions. What is the volume of this new container?

27. original volume (V 1 ) = 40 mL final volume (V 2 ): to be determined CLICK TO CONTINUE LISTEN THOUGHTFULLY GO AT YOUR OWN PACE MAKE NOTES AS NECESSARY (ANALYSIS OF THE PROBLEM) original pressure (P 1 ) = 800 torrs final pressure (P 2 ) = standard pressure = 760 torrs original temperature (T 1 ) = 30 0C0C final temperature (T 2 ) = standard temperature = 25 0C0C

28. CLICK TO CONTINUE P 1 V 1 = P 2 V 2 T 1 T 2 LISTEN THOUGHTFULLY GO AT YOUR OWN PACE MAKE NOTES AS NECESSARY (ANALYSIS OF THE PROBLEM)

29. When the final volume is determined, it will have the unit of the initial volume; the initial and final pressure units are both given in torrs; the temperature units are changed to Kelvin by adding 273: LISTEN THOUGHTFULLY GO AT YOUR OWN PACE MAKE NOTES AS NECESSARY (ANALYSIS OF THE PROBLEM)

30. 30 o C = (30 + 273) K = 303 K 25 o C = (25 + 273) K = 298 K LISTEN THOUGHTFULLY GO AT YOUR OWN PACE MAKE NOTES AS NECESSARY (UNIT CONVERSION)

31. 800 torrs x 40 mL = 760 torrs x V 2 300 K298 K V 2 = 800 torrs x 40 mL x 298 K 300 K x 760 torrs P 1 V 1 = P 2 V 2 T 1 T 2 CLICK TO CONTINUE LISTEN THOUGHTFULLY GO AT YOUR OWN PACE MAKE NOTES AS NECESSARY (FORMATING THE SOLUTION)

32. V 2 = P 1 V 1 T 2 T 1 P 2 = 800 torrs x 40 mL x 298 K 300 K x 760 torrs P 1 V 1 = P 2 V 2 T 1 T 2 CLICK TO CONTINUE LISTEN THOUGHTFULLY GO AT YOUR OWN PACE MAKE NOTES AS NECESSARY (FORMATING THE SOLUTION)

33. V 2 = 41.8 mL CLICK TO CONTINUE LISTEN THOUGHTFULLY GO AT YOUR OWN PACE MAKE NOTES AS NECESSARY (EVALUATION)

34. Example 3: A pure sample of CO 2 was collected and stored in a 2.5-liter flask on a day when the atmospheric pressure was one atmosphere. The next day when the temperature in the storage area was 27 o C the gas was at a pressure of 776 mm Hg. At what temperature was the gas originally collected? CLICK TO CONTINUE LISTEN THOUGHTFULLY GO AT YOUR OWN PACE MAKE NOTES AS NECESSARY (GAS LAW CALCULATION)

35. original volume (V 1 ) = 2.5 L final volume (V 2 ) = 2.5 L CLICK TO CONTINUE original temperature (T 1 ) = to be determined final temperature (T 2 ) = 27 oCoC LISTEN THOUGHTFULLY GO AT YOUR OWN PACE MAKE NOTES AS NECESSARY (ANALYSIS OF THE PROBLEM) original pressure (P 1 ) = 1.0 atm final pressure (P 2 ) = 776 mm Hg

36. P 1 = P 2 T 1 T 2 CLICK TO CONTINUE LISTEN THOUGHTFULLY GO AT YOUR OWN PACE MAKE NOTES AS NECESSARY (ANALYSIS OF THE PROBLEM)

37. Initial pressure: 1.0 atm = 760 mm Hg CLICK TO CONTINUE Final temperature: 27 o C = (27 + 273) K = 300 K LISTEN THOUGHTFULLY GO AT YOUR OWN PACE MAKE NOTES AS NECESSARY (UNIT CONVERSION)

38. EITHER 760 mm Hg = 776 mm Hg T 1 300 K T 1 = 760 mm Hg x 300 K 776 mm Hg OR T 1 = P 1 T 2 P 2 T 1 = 760 mm Hg x 300 K 776 mm Hg CLICK TO CONTINUE LISTEN THOUGHTFULLY GO AT YOUR OWN PACE MAKE NOTES AS NECESSARY (FORMATING THE SOLUTION)

39. T 1 = 294 K T 1 = (294 – 273) oCoC = 21 oCoC CLICK TO CONTINUE LISTEN THOUGHTFULLY GO AT YOUR OWN PACE MAKE NOTES AS NECESSARY (EVALUATION)

40. Example 4: A pure sample of CO 2 was collected at 299 K and stored in a 2.5-liter flask on a day when the atmospheric pressure was 1.04 atmosphere. How much carbon dioxide was collected? CLICK TO CONTINUE LISTEN THOUGHTFULLY GO AT YOUR OWN PACE MAKE NOTES AS NECESSARY (GAS LAW CALCULATION)

41. temperature of gas, T = 299 K volume of gas, V = 2.5 L pressure of gas, P = 1.04 atm amount of gas, n: to be determined Gas law: PV = nRT (IDEAL GAS LAW) CLICK TO CONTINUE LISTEN THOUGHTFULLY GO AT YOUR OWN PACE MAKE NOTES AS NECESSARY (ANALYSIS OF THE PROBLEM)

42. R = 0.082053 L atm mol K CLICK TO CONTINUE LISTEN THOUGHTFULLY GO AT YOUR OWN PACE MAKE NOTES AS NECESSARY (ANALYSIS OF THE PROBLEM)

43. EITHER 1.04 atm x 2.5 L = n x 0.082053 atm L x 299 K mol K n = 1.04 atm x 2.5 L 0.082053 atm L mol -1 K -1 x 299 K OR n = PV RT n = 1.04 atm x 2.5 L 0.082053 atm L mol -1 K -1 x 299 K CLICK TO CONTINUE LISTEN THOUGHTFULLY GO AT YOUR OWN PACE MAKE NOTES AS NECESSARY (FORMATING THE SOLUTION)

44. n = 0.106 mol CLICK TO CONTINUE LISTEN THOUGHTFULLY GO AT YOUR OWN PACE MAKE NOTES AS NECESSARY (EVALUATION)

45. mass of carbon dioxide = n x molar mass = 0.106 mol x 44.010 g/mol = 4.67 g CLICK TO CONTINUE LISTEN THOUGHTFULLY GO AT YOUR OWN PACE MAKE NOTES AS NECESSARY (FORMATING, EVALUATION)

46. volume of carbon dioxide = n x molar volume at S.T.P. = 0.106 mol CO 2 x 22.414 L/mol = 2.38 L CO 2 at S.T.P. CLICK TO CONTINUE LISTEN THOUGHTFULLY GO AT YOUR OWN PACE MAKE NOTES AS NECESSARY (FORMATING, EVALUATION)

47. END OF TUTORIAL SUMMARY OF GAS LAWS Gas LawEquation Avagadro’sn/V 1 = n/V 2 Boyle’sP 1 V 1 = P 2 V 2 Charles’V 1 /T 1 = V 2 /T 2 CombinedP 1 V 1 /T 1 = P 2 V 2 /T 2 Dalton’sP tot = P 1 + P 2 + P 3 +… Gay-Lussac’sP 1 /T 1 = P 2 /T 2 IdealPV = nRT CLICK TO CONTINUE

48. RETURN TO TUTORIAL CLOSE AND GO TO POST-QUIZ OR