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GASES

GASES. Importance of Gases. Airbags fill with N 2 gas in an accident. Gas is generated by the decomposition of sodium azide, NaN 3 . 2 NaN 3  2 Na + 3 N 2 The air we breathe. THREE STATES OF MATTER. General Properties of Gases. There is a lot of “free” space in a gas.

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GASES

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  1. GASES

  2. Importance of Gases • Airbags fill with N2 gas in an accident. • Gas is generated by the decomposition of sodium azide, NaN3. • 2 NaN3 2 Na + 3 N2 • The air we breathe

  3. THREE STATES OF MATTER

  4. General Properties of Gases • There is a lot of “free” space in a gas. • Gases can be expanded infinitely. • Gases fill containers uniformly and completely. • Gases diffuse and mix rapidly.

  5. Properties of Gases Gas properties can be modeled using math. Model depends on— • V = volume of the gas (L)= vol. of container • T = temperature (Kelvin) (K) • ALL temperatures in the entire chapter MUST be in Kelvin!!! No Exceptions! • n = amount (moles) • P = pressure (atmospheres)

  6. Pressure Pressure of air is measured with a BAROMETER Hg rises in tube until force of Hg (down) balances the force of atmosphere (pushing up). (Just like a straw in a soft drink) P of Hg pushing down related to • Hg density • column height

  7. Pressure Column height measures Pressure of atmosphere • 1 standard atmosphere (atm) = 760 mm Hg = 760 torr = 101.3 kPa (SI unit is PASCAL) = 101,300 Pascals

  8. Pressure Conversions A. What is 475 mm Hg expressed in atm? 760 mm Hg = 1 atm 475 mm Hg = x x = 475/760 = 0.625 atm B. The pressure of a tire is measured as 10 kPa. What is this pressure in mm Hg?

  9. Pressure Conversions A. What is 2 atm expressed in torr?

  10. Boyle’s Law Robert Boyle (1627-1691). Son of Early of Cork, Ireland. • Relationship between Pressure and volume keeping the other variables constant. • How does the pressure of a gas behaves when the volume is changed? • P goes up as V goes down. • This means Pressure and Volume are INVERSELY PROPORTIONAL if moles and temperature are constant. • P  1/V • PV = constant • P1V1 = P2 V2

  11. Boyle’s Law A bicycle pump is a good example of Boyle’s law. As the volume of the air trapped in the pump is reduced, its pressure goes up, and air is forced into the tire.

  12. Boyles  Graphs PV Volume (L)

  13. Boyles law questions SCH3U   Boyle's Law Worksheet           1.    State the pressure-volume law both in words and in the form of an equation.2.To compress nitrogen at 1 atm from 750 mL to 500 mL, what must the new pressure be  if the temperature is kept constant? 1.5 atm 3.If oxygen at 128 kPa is allowed to expand at constant temperature until its pressure is 101.3 kPa, how much larger will the volume become? 1.26 4.A sample of nitrogen at 101.3 kPa with a volume of 100 mL is carefully compressed at constant temperature in successive changes in pressure, equalling 5 kPa at a time, until the final pressure is 133.3 kPa. Calculate     each new volume and prepare a plot of P versus V, showing P on the horizontal axis. 5.A sample of nitrogen at 20oC was compressed from 300 mL to 0.360 mL and its new pressure was found to be 400.0 Pa. What was the original pressure in kPa?4.8 x 10-4 6.The pressure on 6.0 L of a gas is 200 kPa. What will be the volume if the pressure is doubled, keeping the temperature constant?3L 7.What would be the new volume if the pressure on 600 mL is increased from 90 kPa to 150 kPa? 360 mL 8.A student collects 25 mL of gas at 96 kPa. What volume would this gas occupy at 101.325 kPa. There is no change in temperature or mass. 23.68 mL 9.A gas measuring 525 mL is collected at 104.66 kPa. What volume does this gas occupy at 99.33 kPa?553.17 mL 10. A mass of gas occupies 1 L at 1 atm. At what pressure does this gas occupya) 2 litres, 0.5 atmb) 0.5 litres? 2 atm 11.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 =  2.8 L 8 atmb)    V1 = 60 mL;   P1 = ? kPa;   P2 = 101.3 kPa;  V2 = 16 mL 27 kPac)     V1 = ? m3 ;    P1 = 40 Pa;   P2 = 100 kPa;  V2 = 1.0 L 2500 L= 2.5 x 109 m3 d)    V1 = 2.50 L;   P1 = 7.5 atm;   P2 = ? atm;  V2 = 100 mL 187.5 atm

  14. Charles’ Law Jacques Charles (1746-1823). Isolated boron and studied gases. Balloonist. • Relationship between volume and Temperature keeping n and P constant. • V and T are directly proportional. • V  T in Kelvin • V/T is a constant • V1/T1 = V2/T2 • If one temperature goes up, the volume goes up!

  15. Charles’s Law Graph Absolute Zero 0 Kelvin = -273.15 0C

  16. SCH3U     Charles Law Worksheet       • Give the temperature-volume law both in words and in the form of an equation. • How is the volume of a gas affected by a decrease in temperature? • What would be the new volume if the temperature on 450 mL of gas is changedfrom 45oC to - 5oC 379 mL • A  sample of gas whose volume at 27oC is 0.127 L, is heated at constant pressureuntil its volume becomes 317 mL. What is the final temperature of the gas in Celsiusand kelvin? • To make 300 mL of oxygen at 20.0oC change its volume to 250 mL, what must bedone to the sample if its pressure and mass are to be held constant? • To what temperature must an ideal gas at 27oC be cooled to reduce its volume to 1/3? • From the data in the following questions calculate the missing quantity.a) V1 = 22.4 L;    T1 = 0oC;  T2 = 91oC;  V2 = ? Lb) V1 = 125 mL;  T1 = ? ;      T2 = 25oC;  V2 = 100 mLc) V1 =  ? L;  T1 = 400 K;  T2 = 175 K;  V2 = 6.20 Ld) V1 = 250 mL;   T1 = 298 K;  T2 = ? K;  V2 = 273 mL • A 50 cm3 sample of a gas in a syringe at 15oC is heated to 50oC and the syringe'spiston is allowed to move outward against a constant atmospheric pressure. Calculatethe new volume of the hot gas. • What is the final volume if 3.4 L of nitrogen gas at 400 K is cooled to 200 K andkept at the same pressure? • Determine the final volume of 20 L of a gas whose temperature changes from -73oCto 327oC if the pressure remains constant. • A partially filled plastic balloon contains 3.4 x 103 m3 of helium gas at 5oC. Thenoon day sun heats this gas to 37oC. What is the volume of the balloon ifatmospheric pressure remains constant?

  17. Gay-Lussac’s Law Joseph Louis Gay-Lussac (1778-1850) • Relationship between P and T keeping moles and volume constant • Pressure increase, temperature increase • P and T are directly proportional. • P α T • P/T = constant • P1 / T1 = P2 / T2

  18. Combined Gas Law • The good news is that you don’t have to remember all three gas laws! Since they are all related to each other, we can combine them into a single equation. • BE SURE YOU KNOW THIS EQUATION! P1 V1 / T1 = P2 V2 / T2

  19. Combined Gas Law If you should only need one of the other gas laws, you can cover up the item that is constant and you will get that gas law! = P1 V1 P2 Boyle’s Law Charles’ Law Gay-Lussac’s Law V2 T1 T2

  20. Combined Gas Law Problem A sample of helium gas has a volume of 0.180 L, a pressure of 0.800 atm and a temperature of 29°C. What is the new temperature(°C) of the gas at a volume of 90.0 mL and a pressure of 3.20 atm? Set up Data Table P1 = 0.800 atm V1 = 0.180 L = 180 mL T1 = 29 + 273 = 302 K P2 = 3.20 atm V2= 90 mL T2 = ??

  21. Calculation P1 = 0.800 atm V1 = 180 mL T1 = 302 K P2 = 3.20 atm V2= 90 mL T2 = ?? P1 V1 P2 V2 = P1 V1 T2 = P2 V2 T1 T1 T2 T2 = P2 V2 T1 P1 V1 T2 = 3.20 atm x 90.0 mL x 302 K 0.800 atm x 180.0 mL T2 = 604 K - 273 = 331 °C = 604 K

  22. Learning Check A gas has a volume of 675 mL at 35°C and 0.850 atm pressure. What is the temperature in °C when the gas has a volume of 0.315 L and a pressure of 802 mm Hg?

  23. Combined gas law worksheet 1.     Helium in a 100 mL container at a pressure of 66.6 kPa is transferred to a container with a volume of 250 mL. What is the new pressure if no change in temperature occurs?  What is the new pressure if the temperature changes from 20oC to 15oC? 2.What will have to happen to the temperature of a sample of methane if 1000 mL at 98.6 kPa and 25oC is given a pressure of 108.5 kPa and a volume of 900 mL? 3.A gas has a volume of 225 mL at 75oC and 175 kPa. What will be its volume at a temperature of 20oC and a pressure of 1.0 X 105 kPa? 4.A gas is heated to 80oC and a pressure of 180 kPa. If the container expands to hold a volume of 800 mL, what was the volume of the gas, (in litres), at a temperature of 50oC and 120 kPa pressure? 5.A 200 mL sample of gas is collected at 50 kPa and a temperature of 271oC.  What volume would this gas occupy at 100 kPa and a temperature of -14oC? 6.Correct the following volumes at STP and at SATP:(a)  24.6 L at 25oC and 104 kPa                (b)  150000 mm3 at 100oC and 75.00 kPa(c)   0.045 L at -45.0oC and 140.0 kPa     (d)   0.5 L at 115oC and 148000 Pa 7.A certain sample of gas has a volume of 0.452 L measured at 87oC and 0.620 atm.  What is its volume at 1 atm and 0oC? 8. Natural gas is usually stored in large underground reservoirs or in above ground  tanks. Suppose that a supply of natural gas is stored in an underground reservoir of volume 8.0 X 105 m3 at a pressure of 360 kPa and a temperature of 16oC. How many above ground tanks of volume 2.7 X 104 m3 at a temperature of 6oC could be filled with the gas at a pressure of 120 kPa? 9.The human lung has an average temperature of 37oC.  If one inhales Alaskan air at 1 atm and -28.9oC and then holds it, to what pressure will the air in the lungs rise? (The bursting strength of the human lung is over 2 atm.  Will they burst?) 10. A cylindrical coffee can is welded shut at 20oC at sea level.  Its height is 20 cm and its radius is 15 cm. If the bursting strength of it's "tin" plate is 3.75 atm, to what temperature may it be heated before bursting?

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