CH104 Chapter 7 Gases Gases & Kinetic Theory Pressure Gas Laws.
Gas Laws Chapter 14 (last one!!) Kinetic Molecular Theory helps explain why gases behave differently...
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Transcript of Gas Laws Chapter 14 (last one!!) Kinetic Molecular Theory helps explain why gases behave differently...
![Page 1: Gas Laws Chapter 14 (last one!!) Kinetic Molecular Theory helps explain why gases behave differently than solids and liquids Gases…. 1. Gas particles do.](https://reader030.fdocuments.us/reader030/viewer/2022032707/56649e4d5503460f94b42cec/html5/thumbnails/1.jpg)
Gas LawsChapter 14 (last one!!)
• Kinetic Molecular Theory helps explain why gases behave differently than solids and liquids
• Gases….
1. Gas particles do not attract nor repel each other
![Page 2: Gas Laws Chapter 14 (last one!!) Kinetic Molecular Theory helps explain why gases behave differently than solids and liquids Gases…. 1. Gas particles do.](https://reader030.fdocuments.us/reader030/viewer/2022032707/56649e4d5503460f94b42cec/html5/thumbnails/2.jpg)
Kinetic Molecular Theory
2. Gas particles are much smaller than the distances between them. This is why gases are compressible.
![Page 3: Gas Laws Chapter 14 (last one!!) Kinetic Molecular Theory helps explain why gases behave differently than solids and liquids Gases…. 1. Gas particles do.](https://reader030.fdocuments.us/reader030/viewer/2022032707/56649e4d5503460f94b42cec/html5/thumbnails/3.jpg)
Kinetic Molecular Theory
3. Gas particles are in constant random motion and they quickly become mixed in a closed container.
![Page 4: Gas Laws Chapter 14 (last one!!) Kinetic Molecular Theory helps explain why gases behave differently than solids and liquids Gases…. 1. Gas particles do.](https://reader030.fdocuments.us/reader030/viewer/2022032707/56649e4d5503460f94b42cec/html5/thumbnails/4.jpg)
Kinetic Molecular Theory
4. Collisions between gas particles or the sides of the container are totally elastic. There is no kinetic energy lost
![Page 5: Gas Laws Chapter 14 (last one!!) Kinetic Molecular Theory helps explain why gases behave differently than solids and liquids Gases…. 1. Gas particles do.](https://reader030.fdocuments.us/reader030/viewer/2022032707/56649e4d5503460f94b42cec/html5/thumbnails/5.jpg)
Kinetic Molecular Theory
5. If at the same temperature, all gases will have the same kinetic energy
temperature = measure of the average kinetic energy
![Page 6: Gas Laws Chapter 14 (last one!!) Kinetic Molecular Theory helps explain why gases behave differently than solids and liquids Gases…. 1. Gas particles do.](https://reader030.fdocuments.us/reader030/viewer/2022032707/56649e4d5503460f94b42cec/html5/thumbnails/6.jpg)
Standard Temperature and Pressure (STP)
• Normal conditions– 0°C
• °C + 273 = Kelvin
– 1 atm= 14.7 psi
= 101.3 kPa
= 760 mmHg
![Page 7: Gas Laws Chapter 14 (last one!!) Kinetic Molecular Theory helps explain why gases behave differently than solids and liquids Gases…. 1. Gas particles do.](https://reader030.fdocuments.us/reader030/viewer/2022032707/56649e4d5503460f94b42cec/html5/thumbnails/7.jpg)
• Overall, the Kinetic Molecular Theory is based on four variables
1. Temperature
2. Pressure
3. Volume
4. Number of Particles
• We can use gas laws to describe these changes.
![Page 8: Gas Laws Chapter 14 (last one!!) Kinetic Molecular Theory helps explain why gases behave differently than solids and liquids Gases…. 1. Gas particles do.](https://reader030.fdocuments.us/reader030/viewer/2022032707/56649e4d5503460f94b42cec/html5/thumbnails/8.jpg)
You’ll be able to use…
1. Boyle’s Law• Pressure & Volume
2. Charles’s Law• Volume & Temperature
3. Gay-Lussac’s Law• Pressure & Temperature
4. Combined Gas Law• Pressure, Volume, & Temperature
5. Graham’s Law of Diffusion
![Page 9: Gas Laws Chapter 14 (last one!!) Kinetic Molecular Theory helps explain why gases behave differently than solids and liquids Gases…. 1. Gas particles do.](https://reader030.fdocuments.us/reader030/viewer/2022032707/56649e4d5503460f94b42cec/html5/thumbnails/9.jpg)
Boyle’s Law• If pressure on a gas was doubled, the
volume of gas decreased by half
• Inverse relationship = one goes up, the other goes down
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Boyle’s Law• Helps explain how we breathe
– As our ribs and diaphragm give lungs more room to move (increase volume) the pressure is lowered and air comes into our lungs
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Units of Pressure• All of these are based on atmospheres.
• Sea level = 1 atmosphere =• =14.7 psi (pounds per square inch)• =101.3 kPa (kilo Pascals)• = 760 mmHg (millimeter of mercury)
![Page 12: Gas Laws Chapter 14 (last one!!) Kinetic Molecular Theory helps explain why gases behave differently than solids and liquids Gases…. 1. Gas particles do.](https://reader030.fdocuments.us/reader030/viewer/2022032707/56649e4d5503460f94b42cec/html5/thumbnails/12.jpg)
Boyle’s Law
• If a gas occupies 2 Liters at 1 atm, what will be the volume of this gas at 4 atm?
P1V1 = P2V2
2 L (1 atm) = X (4 atm)
2 = 4 X
X = 0.5 Liters
![Page 13: Gas Laws Chapter 14 (last one!!) Kinetic Molecular Theory helps explain why gases behave differently than solids and liquids Gases…. 1. Gas particles do.](https://reader030.fdocuments.us/reader030/viewer/2022032707/56649e4d5503460f94b42cec/html5/thumbnails/13.jpg)
Practice Boyle’s Law I1. Convert 202.6 kPa to psi
2. Convert 500 mmHg to kPa
3. Convert 100 psi to mmHg
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Practice Boyle’s Law I4. Convert 3 atm to mmHg
5. Convert 50 psi to mmHg
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Practice Boyle’s Law I6. If a gas occupies 2.56 L at 1 atm, what
will be the volume of this gas at 2 atm?
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Practice Boyle’s Law I7. If 600 mL of a gas is at a pressure of 9
atm, what will be the volume at 3 atm?
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Practice Boyle’s Law I8. If 200 mL of O2 is collected at a pressure
of 5 atm, what volume will this gas occupy at STP?
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Practice Boyle’s Law I9. A gas occupies a volume of 500 mL at
101.3 kPa. What volume will it occupy at 400 kPa?
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Practice Boyle’s Law I10. A gas occupies one liter at STP. How
much pressure (atm) would be required to decrease the volume to 100 mL?
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Practice Boyle’s Law I11. If a gas occupies 1500 mL at 303.9 kPa,
how many atmospheres of pressure will be needed to reduce its volume to 500 mL?
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Practice Boyle’s Law I12. If the pressure of 500 mL of a gas
changes from 800 mmHg to 120 psi, what will be the new volume?