GasGrade 10 MYP
Gasof the4 postulatesKinetic Theory ofGases:
Gasof the4 postulatesKinetic Theory ofGases:4 factors whichdictate howgases behave:1.temperature  (T)2.pressure (P)3.volum...
Gas4 factors whichdictate howgases behave:1.temperature  (T)2.pressure (P)3.volume (V)4.amount (n) How do each of these fa...
GasHow do each of these factors impact             This is              gases?             called      ZERO particle      ...
GasHow do each of these factors impact             gases?
Gas of these factors impactHow do each            gases?
Gas of these factors impactHow do each                  gases?4 factors whichdictate howgases behave:1.temperature  (T)2.p...
Gas of these factors impactHow do each                gases?2.pressure  (P)  measured  in Pascals  (Pa) or kPa
Gas of these factors impactHow do each                gases?                    Force is related to KE!                   ...
Gas of these factors impactHow do each            gases?
Gas of these factors impactHow do each                  gases?4 factors whichdictate howgases behave:1.temperature  (T)2.p...
Gas of these factors impactHow do each                   gases?                                    V  smaller volume = les...
Gas of these factors impactHow do each            gases?
Gas of these factors impactHow do each                  gases?4 factors whichdictate howgases behave:1.temperature  (T)2.p...
Gas of these factors impactHow do each                    gases?4.amount (n)  measured  in moles  more moles = more       ...
Gas  Let’s review    all these  relationship        s...
Gas  Let’s review    all these  relationship        s...
Gas
Gas
Gas   Pressure and Volumeif             ThisP...           isthen               INVERSEV...It is         Expressedalso    ...
Gas   Pressure and Volume       P1V1 = P2V2P1 = starting   P2 = endingV1 = starting   V2 = ending         Boyle’s
Gas
GasTemperature and Volumeif           ThisT...then         is             DIRECT.V...It is        Expressedalso         as...
GasTemperature and Volume     V1/T1 = V2/ V1 = starting   V2 = ending T1 = starting   T2 = ending        Charles’
Gas      V1/T1 = V2/
Gas      V1/T1 = V2/
Gas          How do Charles’                and Boyle’s laws                work TOGETHER?V1/T1 = V2/           P1V1 =P1V1...
Gas
Gas   Finally, one last gas    law...
Gas
Gas
Gas     The IDEALPV = nRT gas law PV nRT pressure(Pa)volume(m 3)moles(mol)consta        R = 8.314 J/nttemperature      K*m...
Gas
Gas
Gas      In summary:Boyle’s       P1V1 =Charles’      V1/T1 =              P1V1 =Combined              T1     T2          ...
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Gas laws

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I created this presentation for my 10th grade MYP science class's unit on energy and change in chemistry. It's just an introduction to the relationships described by gas law formulas but does not go into detail about how to solve them.

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  • Kinetic Theory of Gases\nFactors affecting gas behavior\n
  • Kinetic Theory of Gases\nFactors affecting gas behavior\n
  • Kinetic Theory of Gases\nFactors affecting gas behavior\n
  • Kinetic Theory of Gases\nFactors affecting gas behavior\n
  • Kinetic Theory of Gases\nFactors affecting gas behavior\n
  • Kinetic Theory of Gases\nFactors affecting gas behavior\n
  • Kinetic Theory of Gases\nFactors affecting gas behavior\n
  • Kinetic Theory of Gases\nFactors affecting gas behavior\n
  • Kinetic Theory of Gases\nFactors affecting gas behavior\n
  • Temperature = KE\nKelvins\nAbsolute zero\n
  • Temperature = KE\nKelvins\nAbsolute zero\n
  • Temperature = KE\nKelvins\nAbsolute zero\n
  • Temperature = KE\nKelvins\nAbsolute zero\n
  • Temperature = KE\nKelvins\nAbsolute zero\n
  • Temperature = KE\nKelvins\nAbsolute zero\n
  • Temperature = KE\nKelvins\nAbsolute zero\n
  • Temperature = KE\nKelvins\nAbsolute zero\n
  • Temperature = KE\nKelvins\nAbsolute zero\n
  • Temperature = KE\nKelvins\nAbsolute zero\n
  • Temperature = KE\nKelvins\nAbsolute zero\n
  • Temperature = KE\nKelvins\nAbsolute zero\n
  • Temperature = KE\nKelvins\nAbsolute zero\n
  • Temperature = KE\nKelvins\nAbsolute zero\n
  • Temperature = KE\nKelvins\nAbsolute zero\n
  • Temperature = KE\nKelvins\nAbsolute zero\n
  • Temperature = KE\nKelvins\nAbsolute zero\n
  • Temperature = KE\nKelvins\nAbsolute zero\n
  • Temperature = KE\nKelvins\nAbsolute zero\n
  • Temperature = KE\nKelvins\nAbsolute zero\n
  • Temperature = KE\nKelvins\nAbsolute zero\n
  • Temperature = KE\nKelvins\nAbsolute zero\n
  • measured in Pascals (Pa) or kPa\nPressure = Force/Area\nP and F = directly proportional\nP and A = inversely proportional\n
  • measured in Pascals (Pa) or kPa\nPressure = Force/Area\nP and F = directly proportional\nP and A = inversely proportional\n
  • measured in Pascals (Pa) or kPa\nPressure = Force/Area\nP and F = directly proportional\nP and A = inversely proportional\n
  • measured in Pascals (Pa) or kPa\nPressure = Force/Area\nP and F = directly proportional\nP and A = inversely proportional\n
  • measured in Pascals (Pa) or kPa\nPressure = Force/Area\nP and F = directly proportional\nP and A = inversely proportional\n
  • measured in Pascals (Pa) or kPa\nPressure = Force/Area\nP and F = directly proportional\nP and A = inversely proportional\n
  • measured in Pascals (Pa) or kPa\nPressure = Force/Area\nP and F = directly proportional\nP and A = inversely proportional\n
  • measured in Pascals (Pa) or kPa\nPressure = Force/Area\nP and F = directly proportional\nP and A = inversely proportional\n
  • measured in Pascals (Pa) or kPa\nPressure = Force/Area\nP and F = directly proportional\nP and A = inversely proportional\n
  • measured in Pascals (Pa) or kPa\nPressure = Force/Area\nP and F = directly proportional\nP and A = inversely proportional\n
  • measured in Pascals (Pa) or kPa\nPressure = Force/Area\nP and F = directly proportional\nP and A = inversely proportional\n
  • Volume\nP + V are inversely proportional\n
  • Volume\nP + V are inversely proportional\n
  • Volume\nP + V are inversely proportional\n
  • Volume\nP + V are inversely proportional\n
  • Volume\nP + V are inversely proportional\n
  • Volume\nP + V are inversely proportional\n
  • Volume\nP + V are inversely proportional\n
  • Volume\nP + V are inversely proportional\n
  • Amount = moles\nremember Avogadro = 6.02e23! \n
  • Amount = moles\nremember Avogadro = 6.02e23! \n
  • Amount = moles\nremember Avogadro = 6.02e23! \n
  • Amount = moles\nremember Avogadro = 6.02e23! \n
  • Amount = moles\nremember Avogadro = 6.02e23! \n
  • Amount = moles\nremember Avogadro = 6.02e23! \n
  • Amount = moles\nremember Avogadro = 6.02e23! \n
  • Amount = moles\nremember Avogadro = 6.02e23! \n
  • Amount = moles\nremember Avogadro = 6.02e23! \n
  • Amount = moles\nremember Avogadro = 6.02e23! \n
  • Amount = moles\nremember Avogadro = 6.02e23! \n
  • Amount = moles\nremember Avogadro = 6.02e23! \n
  • Amount = moles\nremember Avogadro = 6.02e23! \n
  • Amount = moles\nremember Avogadro = 6.02e23! \n
  • \n
  • Boyle’s Law: pressure and volume\ninverse relationship\n
  • Boyle’s Law: pressure and volume\ninverse relationship\n
  • Boyle’s Law: pressure and volume\ninverse relationship\n
  • Boyle’s Law: pressure and volume\ninverse relationship\n
  • Boyle’s Law: pressure and volume\ninverse relationship\n
  • Boyle’s Law: pressure and volume\ninverse relationship\n
  • Boyle’s Law: pressure and volume\ninverse relationship\n
  • Boyle’s Law: pressure and volume\ninverse relationship\n
  • Boyle’s Law: pressure and volume\ninverse relationship\n
  • Boyle’s Law: pressure and volume\ninverse relationship\n
  • Boyle’s Law: pressure and volume\ninverse relationship\n
  • Boyle’s Law: pressure and volume\ninverse relationship\n
  • Boyle’s Law: pressure and volume\ninverse relationship\n
  • Boyle’s Law: pressure and volume\ninverse relationship\n
  • Boyle’s Law: pressure and volume\ninverse relationship\n
  • Boyle’s Law: pressure and volume\ninverse relationship\n
  • Boyle’s Law: pressure and volume\ninverse relationship\n
  • Boyle’s Law: pressure and volume\ninverse relationship\n
  • Boyle’s Law: pressure and volume\ninverse relationship\n
  • Boyle’s Law: pressure and volume\ninverse relationship\n
  • Charles’ Law: Volume and temperature\nV1 = starting volume\nV2 = ending volume\nT1 = starting temp\nT2 = ending temp\n
  • Charles’ Law: Volume and temperature\nV1 = starting volume\nV2 = ending volume\nT1 = starting temp\nT2 = ending temp\n
  • Charles’ Law: Volume and temperature\nV1 = starting volume\nV2 = ending volume\nT1 = starting temp\nT2 = ending temp\n
  • Charles’ Law: Volume and temperature\nV1 = starting volume\nV2 = ending volume\nT1 = starting temp\nT2 = ending temp\n
  • Charles’ Law: Volume and temperature\nV1 = starting volume\nV2 = ending volume\nT1 = starting temp\nT2 = ending temp\n
  • Charles’ Law: Volume and temperature\nV1 = starting volume\nV2 = ending volume\nT1 = starting temp\nT2 = ending temp\n
  • Charles’ Law: Volume and temperature\nV1 = starting volume\nV2 = ending volume\nT1 = starting temp\nT2 = ending temp\n
  • Charles’ Law: Volume and temperature\nV1 = starting volume\nV2 = ending volume\nT1 = starting temp\nT2 = ending temp\n
  • Charles’ Law: Volume and temperature\nV1 = starting volume\nV2 = ending volume\nT1 = starting temp\nT2 = ending temp\n
  • Charles’ Law: Volume and temperature\nV1 = starting volume\nV2 = ending volume\nT1 = starting temp\nT2 = ending temp\n
  • Charles’ Law: Volume and temperature\nV1 = starting volume\nV2 = ending volume\nT1 = starting temp\nT2 = ending temp\n
  • Charles’ Law: Volume and temperature\nV1 = starting volume\nV2 = ending volume\nT1 = starting temp\nT2 = ending temp\n
  • Charles’ Law: Volume and temperature\nV1 = starting volume\nV2 = ending volume\nT1 = starting temp\nT2 = ending temp\n
  • Charles’ Law: Volume and temperature\nV1 = starting volume\nV2 = ending volume\nT1 = starting temp\nT2 = ending temp\n
  • Charles’ Law: Volume and temperature\nV1 = starting volume\nV2 = ending volume\nT1 = starting temp\nT2 = ending temp\n
  • Charles’ Law: Volume and temperature\nV1 = starting volume\nV2 = ending volume\nT1 = starting temp\nT2 = ending temp\n
  • Charles’ Law: Volume and temperature\nV1 = starting volume\nV2 = ending volume\nT1 = starting temp\nT2 = ending temp\n
  • Charles’ Law: Volume and temperature\nV1 = starting volume\nV2 = ending volume\nT1 = starting temp\nT2 = ending temp\n
  • Charles’ Law: Volume and temperature\nV1 = starting volume\nV2 = ending volume\nT1 = starting temp\nT2 = ending temp\n
  • Charles’ Law: Volume and temperature\nV1 = starting volume\nV2 = ending volume\nT1 = starting temp\nT2 = ending temp\n
  • Charles’ Law: Volume and temperature\nV1 = starting volume\nV2 = ending volume\nT1 = starting temp\nT2 = ending temp\n
  • Charles’ Law: Volume and temperature\nV1 = starting volume\nV2 = ending volume\nT1 = starting temp\nT2 = ending temp\n
  • Charles’ Law: Volume and temperature\nV1 = starting volume\nV2 = ending volume\nT1 = starting temp\nT2 = ending temp\n
  • Charles’ Law: Volume and temperature\nV1 = starting volume\nV2 = ending volume\nT1 = starting temp\nT2 = ending temp\n
  • Charles’ Law: Volume and temperature\nV1 = starting volume\nV2 = ending volume\nT1 = starting temp\nT2 = ending temp\n
  • Charles’ Law: Volume and temperature\nV1 = starting volume\nV2 = ending volume\nT1 = starting temp\nT2 = ending temp\n
  • Combined Gas Law\n***T always in K b/c can’t divide by zero degrees C! \n
  • Combined Gas Law\n***T always in K b/c can’t divide by zero degrees C! \n
  • Combined Gas Law\n***T always in K b/c can’t divide by zero degrees C! \n
  • Combined Gas Law\n***T always in K b/c can’t divide by zero degrees C! \n
  • Combined Gas Law\n***T always in K b/c can’t divide by zero degrees C! \n
  • Combined Gas Law\n***T always in K b/c can’t divide by zero degrees C! \n
  • Combined Gas Law\n***T always in K b/c can’t divide by zero degrees C! \n
  • Combined Gas Law\n***T always in K b/c can’t divide by zero degrees C! \n
  • Combined Gas Law\n***T always in K b/c can’t divide by zero degrees C! \n
  • Combined Gas Law\n***T always in K b/c can’t divide by zero degrees C! \n
  • Combined Gas Law\n***T always in K b/c can’t divide by zero degrees C! \n
  • Combined Gas Law\n***T always in K b/c can’t divide by zero degrees C! \n
  • Combined Gas Law\n***T always in K b/c can’t divide by zero degrees C! \n
  • Combined Gas Law\n***T always in K b/c can’t divide by zero degrees C! \n
  • Combined Gas Law\n***T always in K b/c can’t divide by zero degrees C! \n
  • Combined Gas Law\n***T always in K b/c can’t divide by zero degrees C! \n
  • Combined Gas Law\n***T always in K b/c can’t divide by zero degrees C! \n
  • Combined Gas Law\n***T always in K b/c can’t divide by zero degrees C! \n
  • Combined Gas Law\n***T always in K b/c can’t divide by zero degrees C! \n
  • Combined Gas Law\n***T always in K b/c can’t divide by zero degrees C! \n
  • Combined Gas Law\n***T always in K b/c can’t divide by zero degrees C! \n
  • Combined Gas Law\n***T always in K b/c can’t divide by zero degrees C! \n
  • Combined Gas Law\n***T always in K b/c can’t divide by zero degrees C! \n
  • Combined Gas Law\n***T always in K b/c can’t divide by zero degrees C! \n
  • \n
  • Ideal Gas Law ties together Charles and Boyle’s Laws\n
  • Ideal Gas Law ties together Charles and Boyle’s Laws\n
  • Ideal Gas Law ties together Charles and Boyle’s Laws\n
  • Ideal Gas Law ties together Charles and Boyle’s Laws\n
  • Ideal Gas Law ties together Charles and Boyle’s Laws\n
  • Ideal Gas Law ties together Charles and Boyle’s Laws\n
  • Ideal Gas Law ties together Charles and Boyle’s Laws\n
  • Ideal Gas Law ties together Charles and Boyle’s Laws\n
  • Ideal Gas Law ties together Charles and Boyle’s Laws\n
  • Ideal Gas Law ties together Charles and Boyle’s Laws\n
  • Ideal Gas Law ties together Charles and Boyle’s Laws\n
  • Ideal Gas Law ties together Charles and Boyle’s Laws\n
  • Ideal Gas Law ties together Charles and Boyle’s Laws\n
  • Ideal Gas Law ties together Charles and Boyle’s Laws\n
  • Ideal Gas Law ties together Charles and Boyle’s Laws\n
  • Ideal Gas Law ties together Charles and Boyle’s Laws\n
  • Ideal Gas Law ties together Charles and Boyle’s Laws\n
  • Ideal Gas Law ties together Charles and Boyle’s Laws\n
  • Ideal Gas Law ties together Charles and Boyle’s Laws\n
  • Ideal Gas Law ties together Charles and Boyle’s Laws\n
  • Ideal Gas Law ties together Charles and Boyle’s Laws\n
  • Ideal Gas Law ties together Charles and Boyle’s Laws\n
  • Ideal Gas Law ties together Charles and Boyle’s Laws\n
  • Ideal Gas Law ties together Charles and Boyle’s Laws\n
  • Ideal Gas Law ties together Charles and Boyle’s Laws\n
  • Ideal Gas Law ties together Charles and Boyle’s Laws\n
  • Ideal Gas Law ties together Charles and Boyle’s Laws\n
  • Ideal Gas Law ties together Charles and Boyle’s Laws\n
  • Ideal Gas Law ties together Charles and Boyle’s Laws\n
  • Ideal Gas Law ties together Charles and Boyle’s Laws\n
  • Charles’ Law: Volume and temperature\nV1 = starting volume\nV2 = ending volume\nT1 = starting temp\nT2 = ending temp\n
  • Charles’ Law: Volume and temperature\nV1 = starting volume\nV2 = ending volume\nT1 = starting temp\nT2 = ending temp\n
  • Charles’ Law: Volume and temperature\nV1 = starting volume\nV2 = ending volume\nT1 = starting temp\nT2 = ending temp\n
  • Charles’ Law: Volume and temperature\nV1 = starting volume\nV2 = ending volume\nT1 = starting temp\nT2 = ending temp\n
  • Charles’ Law: Volume and temperature\nV1 = starting volume\nV2 = ending volume\nT1 = starting temp\nT2 = ending temp\n
  • Charles’ Law: Volume and temperature\nV1 = starting volume\nV2 = ending volume\nT1 = starting temp\nT2 = ending temp\n
  • Charles’ Law: Volume and temperature\nV1 = starting volume\nV2 = ending volume\nT1 = starting temp\nT2 = ending temp\n
  • Charles’ Law: Volume and temperature\nV1 = starting volume\nV2 = ending volume\nT1 = starting temp\nT2 = ending temp\n
  • Charles’ Law: Volume and temperature\nV1 = starting volume\nV2 = ending volume\nT1 = starting temp\nT2 = ending temp\n
  • Gas laws

    1. 1. GasGrade 10 MYP
    2. 2. Gasof the4 postulatesKinetic Theory ofGases:
    3. 3. Gasof the4 postulatesKinetic Theory ofGases:4 factors whichdictate howgases behave:1.temperature (T)2.pressure (P)3.volume (V)4.amount (n) How do each of these factors impact gases?
    4. 4. Gas4 factors whichdictate howgases behave:1.temperature (T)2.pressure (P)3.volume (V)4.amount (n) How do each of these factors impact gases?
    5. 5. GasHow do each of these factors impact This is gases? called ZERO particle ABSOLU movement! TE = ZERO! ZERO KE!1.temperature (Which (T) Temperature: ismeasurement of -273.15 What happensAVERAGE random oC) at zero Kelvins? kinetic energy (KE) of all particles; HOT: COLD: measured in high KE = fast low KE = slow Kelvins (K) movement movement
    6. 6. GasHow do each of these factors impact gases?
    7. 7. Gas of these factors impactHow do each gases?
    8. 8. Gas of these factors impactHow do each gases?4 factors whichdictate howgases behave:1.temperature (T)2.pressure (P)3.volume (V)4.amount (n)
    9. 9. Gas of these factors impactHow do each gases?2.pressure (P) measured in Pascals (Pa) or kPa
    10. 10. Gas of these factors impactHow do each gases? Force is related to KE! more KE = more force =if A more Pthen P less KE = less force = less P2.pressure Since KE is related to (P) temperature… measured in Pascals WHAT does that mean (Pa) or kPa about force and temperature? if F then P
    11. 11. Gas of these factors impactHow do each gases?
    12. 12. Gas of these factors impactHow do each gases?4 factors whichdictate howgases behave:1.temperature (T)2.pressure (P)3.volume (V)4.amount (n)
    13. 13. Gas of these factors impactHow do each gases? V smaller volume = less space larger volume = more space P3.volume (V) = more collisions = more less space pressure more space = fewer collisions = less pressure
    14. 14. Gas of these factors impactHow do each gases?
    15. 15. Gas of these factors impactHow do each gases?4 factors whichdictate howgases behave:1.temperature (T)2.pressure (P)3.volume (V)4.amount (n)
    16. 16. Gas of these factors impactHow do each gases?4.amount (n) measured in moles more moles = more fewer moles = fewer (mol) particles particles more particles = more fewer particles = fewer collisions collisions more collisions = more fewer collisions = less
    17. 17. Gas Let’s review all these relationship s...
    18. 18. Gas Let’s review all these relationship s...
    19. 19. Gas
    20. 20. Gas
    21. 21. Gas Pressure and Volumeif ThisP... isthen INVERSEV...It is Expressedalso asBoyle’s P1V1 = P2V2
    22. 22. Gas Pressure and Volume P1V1 = P2V2P1 = starting P2 = endingV1 = starting V2 = ending Boyle’s
    23. 23. Gas
    24. 24. GasTemperature and Volumeif ThisT...then is DIRECT.V...It is Expressedalso asCharles’ V1/T1 = V2/
    25. 25. GasTemperature and Volume V1/T1 = V2/ V1 = starting V2 = ending T1 = starting T2 = ending Charles’
    26. 26. Gas V1/T1 = V2/
    27. 27. Gas V1/T1 = V2/
    28. 28. Gas How do Charles’ and Boyle’s laws work TOGETHER?V1/T1 = V2/ P1V1 =P1V1 = The Com T1 T2 bined Gas L aw! Temp always in K!
    29. 29. Gas
    30. 30. Gas Finally, one last gas law...
    31. 31. Gas
    32. 32. Gas
    33. 33. Gas The IDEALPV = nRT gas law PV nRT pressure(Pa)volume(m 3)moles(mol)consta R = 8.314 J/nttemperature K*mol (I won’t make you(K) memorize this!)
    34. 34. Gas
    35. 35. Gas
    36. 36. Gas In summary:Boyle’s P1V1 =Charles’ V1/T1 = P1V1 =Combined T1 T2 PV =Ideal Gas nRT
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