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Bell work January 31 st , 2014

Bell work January 31 st , 2014. You will have to do stoichiometry again towards the end of this unit . So, given the following equation, C 3 H 8 + O 2  CO 2 + H 2 O if you start with 10 grams of t ricarbon octahydride , how many grams of water will you end up with?. Agenda.

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Bell work January 31 st , 2014

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  1. Bell workJanuary 31st, 2014 • You will have to do stoichiometry again towards the end of this unit  • So, given the following equation, • C3H8 + O2 CO2 + H2O if you start with 10 grams of tricarbonoctahydride, how many grams of water will you end up with?

  2. Agenda Pressure Conversion Factors Review of the characteristics of gases Objective: You will be able to convert between different units of pressure on your own.

  3. Pressure Videos Basketball: http://www.youtube.com/watch?v=t-Iz414g-ro Egg: http://www.youtube.com/watch?v=28TIyWdfxxc&list=PLCA9B7D3D7031D919

  4. Force Area Barometer Pressure Pressure = For example: 1 pascal (Pa) = 1 N/m2

  5. Write down the following conversion factors: 1 atm = 760 torr 1 atm = 101.3 kPa 1 atm = 760 mmHg 1 atm= 14.7 psi 1 kPa = 7.50 mmHg

  6. As a class… Convert: 1) 727 mmHg into kPa 727mmHg x_1 kPa____ 7.50mmHg 2) 52.5 kPa into atm 3) 0.729 atm into mmHg = 96.9 kPa

  7. Solutions… = 96.9 kPa Convert: 1) 727mmHg x _1 kPa____ 7.50mmHg 2) 52.5 kPax _1 atm___ 101.3 kPa 3) 0.729 atm x _760 mmHg 1 atm = 0.52 atm = 554.0 mmHg

  8. On your own… Convert: 4) 522 torr into kPa 5) 800.0 mmHg into atm 6) 495 kPa into mmHg

  9. Solutions… = 69.58 kPa Convert: 4. 522 torr x _1 atm_x 101.3 kPa 760 torr 1 atm 5. 800.0 mmHg x _1 atm___ 760 mmHg 6. 495 kPa x _7.50 mmHg_ 1 kPa = 1.05 atm = 3712.5 mmHg

  10. Practice If a paint ball CO2 tank is at a pressure of 2000psiand you know that 1psiequals51.7mmHg, how many atm of pressure are in the tank?

  11. Solution Known quantity: 2000 psi Conversion factors: 51.7 mmHg/1 psi 1 atm/760 mmHg

  12. Elements that exist as gases at 250C and 1 atm

  13. Physical Characteristics of Gases Gases assume the volume and shape of their containers. Gases are the most compressible state of matter. Gases will mix evenly and completely when confined to the same container. Gases have much lower densities than liquids and solids.

  14. Standard Temperature and Pressure Standardtemperature and pressure, (STP), refers to conditions in the atmosphere at sea level. Temperature = 0°C or 273K Pressure = 1atm This is essentially the freezing point of pure water at sea level, in air, at standard pressure

  15. Kelvin When doing gas law problems, all temperatures must be in Kelvin, not Celsius! To convert from Celsius to Kelvin, just add 273. So, -10°C would be: -10°C + 273= 263K

  16. Pressure Conversion HW… Convert: 1. 258 mmHg into kPa 2. 30.5 kPa into atm 3. .259 atm into mmHg 4. 752 torr into kPa 5. 526 mmHg into atm 6. 125 kPa into mmHg

  17. Bell Work Feb. 2nd, 2014 Remember density? D = g/ml What is the density of a 5.6 gram substance that takes up 9.8 mL of space. How about volume of a cylinder? Pi*r2h What would be the volume of a sausage link if its diameter was 4 cm and it is 10.2 cm height?

  18. As a class… What is the mass in grams of a textbook that is 10 inches long, 8 inches wide, and 3 inches thick, if it has a density of 0.382 g/cm3?

  19. Remember… Density=mass/volume Volume of a cylinder=pi*r2h

  20. Practice 1. Solve for T2: P1V1 = P2V2 T1 T2 2. What would be the  volume of a 50 gram sphere of platinum (density of platinum = 21.50 g\cm3) 3. What would be the mass of 15.2 cm3 of water? d=1 g/cm3 4. The density of the core of the sun is = 150 g\cm3 how many cubic centimeters would 10 g be? 5. PV = nRT; solve for n! 6. PV = nRT; P=3 atm; V= 1L; T= 273 K; R= .0821atm.L/ mol.K

  21. Practice 1. What would be the  volume of a 50 gram sphere of platinum (density of platinum = 21.50 g\cm3) {ec find the diameter} 2. What would be the mass of 15.2 cm3 of water? 3. What would be the mass in grams, of a solid steel flagpole if its circumference was 20cm? (density of steel = 7.3 g\cm3) *height of 5 meters 4. The density of the core of the sun is = 150 g\cm3 how many cubic centimeters would 10 g be? 5. What would be the mass in grams of the trunk of a tree that had a circumference of 1 meter and was 3 meters tall (density of pine = 600 g\m3) • Solve for T1: P1V1 = P2V2 T1 T2

  22. Bell Work Feb. 3rd, 2014 Not so tough one: What is the pressure of a tank of He in atm if the pressure gauge reads 5700mmHg. Tough one?: What would be the pressure in atm if the pressure gauge read 4500psi and 14.7psi is equals 1 atm?

  23. Bell Work Feb. 3rd, 2014 Not so tough one: What is the pressure of a tank of He in atm if the pressure gauge reads 5700mmHg. Tough one?: What would be the pressure in atm if the pressure gauge read 4500psi and 14.7psi is equals 1 atm?

  24. Extra Credit From test! Using the following equation… HCl + NaOH  H2O + NaCl 1) How many grams of NaCl are produced if you start with 5.5 grams of NaOH? 2) Calculate the percent yield of NaCl if you ended up with 6.5 grams in lab.

  25. Agenda Boyle’s Law Practice Problems Objective: You will know how to carry out basic Boyle’s Gas Law Calculations and visually see the out come on volume when varying pressure.

  26. Videos http://www.youtube.com/watch?v=q6-oyxnkZC0 http://www.youtube.com/watch?v=3yvSQuTP4T4

  27. 10miles 0.2 atm 4 miles 0.5 atm Sea level 1 atm

  28. Open Closed

  29. As P (h) increases V decreases

  30. Boyle’s Law Boyle’s Law Constant temp. Const. amount of gas Pa 1/V P x V = constant P1 x V1 = P2 x V2

  31. What is Boyles Law… P1V1= P2V2 So pressure is inversely proportional to volume: As Pressure goes up… volume goes___ As pressure goes down… volume goes____

  32. Examples of Boyle Law at work A syringe being used to draw blood Popping a balloon Popping ears during elevation change

  33. Solve for … • V2 • P1V1= P2V2 • P1 • P1V1= P2V2

  34. Try this… A sample of chlorine gas occupies a volume of 946mL at a pressure of 726mmHg. What is the pressure of the gas (in mmHg) if the volume is reduced at constant temperature to 154 mL?

  35. = 726 mmHg x 946 mL P1 x V1 154 mL V2 A sample of chlorine gas occupies a volume of 946mL at a pressure of 726mmHg. What is the pressure of the gas (in mmHg) if the volume is reduced at constant temperature to 154 mL? P1 x V1 = P2 x V2 P1 = 726 mmHg P2 = ? V1 = 946 mL V2 = 154 mL P2 = = 4460 mmHg

  36. From the data in the following table calculate the missing quantity (assuming constant temperature). a) V1 = 22.4 L; P1= 1 atm; P2 =? atm; V2 = 2.8L b) V1 = 60mL; P1 =? kPa; P2 = 101.3kPa; V2= 16 mL c)  V1 = ? L ; P1 = 40 kPa;  P2 = 100 kPa;  V2 = 1.0 L d) V1 = 2.50 L; P1 = 7.5 atm; P2 = ?atm; V2 = 0.100L

  37. Practice makes perfect  A sample of hydrogen at 1.50 atm had its pressure decreased to 0.50 atm producing a new volume of 750 mL. What was the sample’s original volume? 250ml

  38. Boyle’s ppt. HW If the initial volume is 3.7 L and the initial pressure is 180.0 KPa, what is the final volume if the final pressure is 160 KPa?  If volume doubles, what happens to pressure? A pressure of 950.0 Kpa is required to initially inflate a balloon 300.0 mL.  What is the final pressure when the balloon has reached its capacity of 1.5 L?

  39. Bellwork 2-4-14 • 1) What happens to volume as pressure increases? • 2) Convert 2.5 atm to kpa. • 3) Now convert that number to mmHg. • 4) What does STP stand for?? • Check your grades—mid quarter is Friday! • Test back to look at—not 5th!

  40. BELL WORK2-5-2014 A sample of mustard gas is in a sealed vessel that can change volume based on internal gas pressure. If the sample of gas started at a volume of 500mL and an unknown pressure and then the pressure changed to 540mmHg and a new volume of 0.75Lwas established, what was the original pressure of the vessel? (write out all the parts first…)

  41. Bell Work6-Feb-2014 Fluorine gas exerts a pressure of 900 torr. When the pressure is changed to 1.50 atm, its volume is 250 mL. What was the original volume? What is 50 degrees C in Kelvin? 78 kpa is equal to how many torr?

  42. Boyle’s Law Lab Please do not damage the plunger/ syringe

  43. Practice makes perfect  1.00L of a gas at standard temperature and pressure is compressed to 473 mL. What is the new pressure of the gas? In a thermonuclear device, the pressure of 0.050L of gas within the bomb casing reaches 4.0 x 106 atm. When the bomb casing is destroyed by the explosion, the gas is released into the atmosphere where it reaches a pressure of 1.00 atm. What is the volume of the gas after the explosion? 2.11atm 2.0x105L

  44. Agenda Boyles Law Practice Problems Finish Boyle’s law lab Objective You will know how to recognize a Pressure volume problem and understand the concept of Boyle’s law

  45. Bell Work7-Feb-2014 Neon gas exerts a pressure of 2.3 atm. When the pressure is changed to 1.50 atm, its volume is 125 mL. What was the original volume in liters? How do you go from Kelvin to Celsius? One more time, what are the values at STP? Solve Boyle’s Law for P2.

  46. Agenda Volume vs. Temp. Charles law Objective: You will understand the relationship between volume and temperature and how it relates to gas molecules. By the end of the period you will be able to compute basic volume temperature calculations.

  47. Recall… With your partner convert 23,015 Kpa to atm. According to Boyle’s Law what happens to Pressure as volume increases?

  48. As T increases… V increases

  49. Variation of gas volume with temp. at constant pressure. Charles’ & Gay-Lussac’s Law VaT V = constant x T V1 = V2 T1 T2

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