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Needhelpp101

  • one year ago

. If measurements of a gas are 50L and 300 kilopascals and then the gas is measured a second time and found to be 75L, describe what had to happen to the pressure (if temperature remained constant). Include which law supports this observation.

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  1. Photon336
    • one year ago
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    Do you know the ideal gas law?

  2. Needhelpp101
    • one year ago
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    The ideal gas law is the equation of state of a hypothetical ideal gas. It is a good approximation to the behavior of many gases under many conditions, although it has several limitations. It was first stated by Émile Clapeyron in 1834 as a combination of Boyle's law and Charles's law.

  3. Photon336
    • one year ago
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    \[Pv = nRT \] pressure times volume = the number of moles of gas times the gas constant times temperature

  4. Photon336
    • one year ago
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    take a look at this formula, and I'll show you how to manipulate it b/c it's the only thing you'll need for the gases. Now to use this equation we must do two things: To study the change in any two of the variables we must keep one of those variables constant.

  5. Photon336
    • one year ago
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    In our case the relationship is as follows: we keep temperature constant, and when we do that well. we can ignore it in our formula so it becomes like this \[pV = nR \] now nR = the number of moles times the gas constant. we're asked to find the new pressure, when given a volume. So it becomes because we're asked to find the new pressure. \[P _{1}V _{1 } = P _{2}V _{2}\] we assumed that the number of moles nR was constant so we omitted that. this shows us that pressure and volume are inversely proportional if i increase pressure by certain amount, then the volume must go down, if i increase volume by a certain amount i decrease my pressure. This makes sense because picture a sealed container, with some gas. if you decrease the volume, the gas particles have less space to move around, and when that happens they hit the walls of the container more frequently and the total pressure goes up. if you increase the volume, the pressure goes down, b/c more space available to the gas to move round less collisions with the walls of the container, at least that's how i understood it. Now what are we solving for? that's P2 so \[\frac{ P _{1} V _{1}}{ V _{2} } = P _{2}\]

  6. Needhelpp101
    • one year ago
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    @Photon336 Can you please dumb down the answer please?

  7. Needhelpp101
    • one year ago
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    "shorten the answer"

  8. Photon336
    • one year ago
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    okay I can walk you through it. so for pressure and volume \[P _{1}V _{1} = P _{2}V _{2}\] if you start out with say some pressure and volume P1V1 and then you increase your volume your pressure goes down, that's what happened in your problem. but can you see why?

  9. Needhelpp101
    • one year ago
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    no :(

  10. Photon336
    • one year ago
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    @Needhelpp101 for starters picture a container, |dw:1437595340805:dw|

  11. Photon336
    • one year ago
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    say we put a certain amount of gas in that container; what is that gas going to do?

  12. Needhelpp101
    • one year ago
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    take up space......I'm dumb sorry thats why i'm on here :(

  13. Photon336
    • one year ago
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    well the gas particles are going to move around, gases always move around

  14. Photon336
    • one year ago
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    and they are going to hit the walls of the container

  15. Needhelpp101
    • one year ago
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    ok

  16. Photon336
    • one year ago
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    now think of the pressure as like how many times the gas particles hit the container make sense?

  17. Needhelpp101
    • one year ago
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    yes

  18. Photon336
    • one year ago
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    Now think of volume as like how much space is available for our gas to move around

  19. Photon336
    • one year ago
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    |dw:1437595907989:dw| if we have something like this what do you see in these two figures

  20. Photon336
    • one year ago
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    What can you say about V1 and V2?

  21. Needhelpp101
    • one year ago
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    hmm...

  22. Photon336
    • one year ago
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    is V1 bigger than V2 or smaller?

  23. Needhelpp101
    • one year ago
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    smaller ?

  24. Photon336
    • one year ago
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    V1 is bigger than V2 let me draw another one

  25. Needhelpp101
    • one year ago
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    k

  26. Photon336
    • one year ago
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    |dw:1437596265405:dw|

  27. Photon336
    • one year ago
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    the way I drew the first one may have been confusing.

  28. Needhelpp101
    • one year ago
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    k

  29. Photon336
    • one year ago
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    what about the one I just drew?

  30. Needhelpp101
    • one year ago
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    V1 is bigger than V2

  31. Photon336
    • one year ago
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    Great

  32. Photon336
    • one year ago
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    now we said a bigger volume = more space available to the gas

  33. Photon336
    • one year ago
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    and pressure = the how many times the gas hits the walls of the container

  34. Photon336
    • one year ago
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    if V1 has a greater volume than V2 then which one would the pressure be greater?

  35. Needhelpp101
    • one year ago
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    V1?

  36. Photon336
    • one year ago
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    another thing if there is less space for the gas to move around that means the gas hits the walls more so more pressure

  37. Needhelpp101
    • one year ago
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    got ya

  38. Photon336
    • one year ago
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    Gases are always moving

  39. Photon336
    • one year ago
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    if there is less space for them to move they will hit the walls more

  40. Needhelpp101
    • one year ago
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    ok

  41. Photon336
    • one year ago
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    so from that figure with the squares which one would have the higher pressure and why?

  42. Needhelpp101
    • one year ago
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    V2 because it's smaller

  43. Needhelpp101
    • one year ago
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    We can use Boyle's Law, pressure is inversely related to volume when temperature is constant P=kV 50=k300 k=50×300=15000 P=15000V now plug in the new volume 75 L P=1500075=200 kilopascals Results: Keeping temperature constant, when you increase the volume the pressure has to decrease. Boyle's law confirms this. For a review of the gas laws http://chemed.chem.purdue.edu/genchem/topicreview/bp/ch4/gaslaws3.html

  44. Photon336
    • one year ago
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    Take a look at this

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  45. Needhelpp101
    • one year ago
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    k

  46. Photon336
    • one year ago
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    That's correct, so do yo understand why that's the case based off what we said?

  47. Needhelpp101
    • one year ago
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    yes :)

  48. Needhelpp101
    • one year ago
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    Can you help me with one question? You make the following measurements of an object – 22 kg and 42 m3. What would the object’s density be? Show your work for credit and include final units.

  49. Photon336
    • one year ago
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    okay one last thing; so for now just think of pressure as how many times the gas hits the walls of the container = pressure volume = how much space gas has to move around. increase volume, more space to move around so gas hits container less, pressure goes down. decrease volume, less space to move around, hits containers more pressure goes up

  50. Photon336
    • one year ago
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    can you put that question in another post? so you got the pressure volume stuff right?

  51. Needhelpp101
    • one year ago
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    yep

  52. JTfan2000
    • one year ago
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    Charles law - volume/temp are related and increasing

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