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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.
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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Photon336
 one year ago
Best ResponseYou've already chosen the best response.1Do you know the ideal gas law?

Needhelpp101
 one year ago
Best ResponseYou've already chosen the best response.0The 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.

Photon336
 one year ago
Best ResponseYou've already chosen the best response.1\[Pv = nRT \] pressure times volume = the number of moles of gas times the gas constant times temperature

Photon336
 one year ago
Best ResponseYou've already chosen the best response.1take 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.

Photon336
 one year ago
Best ResponseYou've already chosen the best response.1In 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 \[\frac{ P _{1} V _{1}}{ V _{2} } = P _{2}\]

Needhelpp101
 one year ago
Best ResponseYou've already chosen the best response.0@Photon336 Can you please dumb down the answer please?

Needhelpp101
 one year ago
Best ResponseYou've already chosen the best response.0"shorten the answer"

Photon336
 one year ago
Best ResponseYou've already chosen the best response.1okay 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?

Photon336
 one year ago
Best ResponseYou've already chosen the best response.1@Needhelpp101 for starters picture a container, dw:1437595340805:dw

Photon336
 one year ago
Best ResponseYou've already chosen the best response.1say we put a certain amount of gas in that container; what is that gas going to do?

Needhelpp101
 one year ago
Best ResponseYou've already chosen the best response.0take up space......I'm dumb sorry thats why i'm on here :(

Photon336
 one year ago
Best ResponseYou've already chosen the best response.1well the gas particles are going to move around, gases always move around

Photon336
 one year ago
Best ResponseYou've already chosen the best response.1and they are going to hit the walls of the container

Photon336
 one year ago
Best ResponseYou've already chosen the best response.1now think of the pressure as like how many times the gas particles hit the container make sense?

Photon336
 one year ago
Best ResponseYou've already chosen the best response.1Now think of volume as like how much space is available for our gas to move around

Photon336
 one year ago
Best ResponseYou've already chosen the best response.1dw:1437595907989:dw if we have something like this what do you see in these two figures

Photon336
 one year ago
Best ResponseYou've already chosen the best response.1What can you say about V1 and V2?

Photon336
 one year ago
Best ResponseYou've already chosen the best response.1is V1 bigger than V2 or smaller?

Photon336
 one year ago
Best ResponseYou've already chosen the best response.1V1 is bigger than V2 let me draw another one

Photon336
 one year ago
Best ResponseYou've already chosen the best response.1dw:1437596265405:dw

Photon336
 one year ago
Best ResponseYou've already chosen the best response.1the way I drew the first one may have been confusing.

Photon336
 one year ago
Best ResponseYou've already chosen the best response.1what about the one I just drew?

Needhelpp101
 one year ago
Best ResponseYou've already chosen the best response.0V1 is bigger than V2

Photon336
 one year ago
Best ResponseYou've already chosen the best response.1now we said a bigger volume = more space available to the gas

Photon336
 one year ago
Best ResponseYou've already chosen the best response.1and pressure = the how many times the gas hits the walls of the container

Photon336
 one year ago
Best ResponseYou've already chosen the best response.1if V1 has a greater volume than V2 then which one would the pressure be greater?

Photon336
 one year ago
Best ResponseYou've already chosen the best response.1another thing if there is less space for the gas to move around that means the gas hits the walls more so more pressure

Photon336
 one year ago
Best ResponseYou've already chosen the best response.1Gases are always moving

Photon336
 one year ago
Best ResponseYou've already chosen the best response.1if there is less space for them to move they will hit the walls more

Photon336
 one year ago
Best ResponseYou've already chosen the best response.1so from that figure with the squares which one would have the higher pressure and why?

Needhelpp101
 one year ago
Best ResponseYou've already chosen the best response.0V2 because it's smaller

Needhelpp101
 one year ago
Best ResponseYou've already chosen the best response.0We 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

Photon336
 one year ago
Best ResponseYou've already chosen the best response.1That's correct, so do yo understand why that's the case based off what we said?

Needhelpp101
 one year ago
Best ResponseYou've already chosen the best response.0Can 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.

Photon336
 one year ago
Best ResponseYou've already chosen the best response.1okay 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

Photon336
 one year ago
Best ResponseYou've already chosen the best response.1can you put that question in another post? so you got the pressure volume stuff right?

JTfan2000
 one year ago
Best ResponseYou've already chosen the best response.0Charles law  volume/temp are related and increasing
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