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Old 25-10-11, 02:49 PM   #1
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Default Chemistry

OK, so there's three syringes. All of them exist at room temperature under one atmosphere of pressure.

First contains 50mL of nitrogen.
Second contains 50ML of oxygen.
Third contains 25mL of carbon dioxide.

You force the oxygen and carbon dioxide into the syringe containing nitrogen. A syringe is basically a container.

Find the pressure in terms of atmospheres. The answer is 2.5, I know this, but how do I calculate it? I need to understand this logic desperately. I know about PV=nRT, but I don't think that would help in this situation because the pressure is in atmospheres, and the number of moles is not given, and the temperature in kelvin is not given. No, Kelvin has not been introduced to my class yet. And no, I don't have a textbook I can rely on. We don't have a textbook. Just our heads. This is why I struggle in this class!








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Last edited by New Evolution; 25-10-11 at 02:52 PM..
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Old 25-10-11, 02:55 PM   #2
 
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Default Re: Chemistry

@Again will help you, she's a chemistry geek

As for me i flopped out of science so Im no use to you




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Old 25-10-11, 02:59 PM   #3
 
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Default Re: Chemistry

I don't even know why I looked at this thread, I suck at all Sciences o_O
Sorry - No clue! Hope you find out soon.









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Old 25-10-11, 03:01 PM   #4
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Default Re: Chemistry

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I don't even know why I looked at this thread, I suck at all Sciences o_O
Sorry - No clue! Hope you find out soon.
Haha well this is chapter 2 of a first year chemistry course, so seems pretty basic to me.








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Old 25-10-11, 03:02 PM   #5
 
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Default Re: Chemistry

Lol now I feel really dumb









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Old 25-10-11, 03:47 PM   #6
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Default Re: Chemistry

I haven't done this is Chemistry yet, so I'm not quite sure how to do it, But I looked up some things. Don't know if the following links will be of any use to you or not...

http://answers.yahoo.com/question/in...2175314AAUPKF7

- This has formulas and things in it..?

http://www.wikihow.com/Calculate-Atmospheric-Pressure

These sound vaugely like what your doing. I might be completely wrong, but this is what I could find. Also, try looking on BBC Bitesize? That's a good site.










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Old 25-10-11, 05:37 PM   #7
 
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Default Re: Chemistry

i think you just use the volumes at one atmosphere and then combine them
add them all together and there is 2.5 times as much in on container, so 2.5 atmospheres
maybe?
i'm not sure though
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Old 25-10-11, 06:05 PM   #8
 
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Default Re: Chemistry

No idea.
You get no books?
I'd be dead x)




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Old 25-10-11, 07:55 PM   #9
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Default Re: Chemistry

You can use density to find the mass of each gas. And from there you can find the moles of each gas. You have T and you have V and You have R. You can find the pressure of each gas from there. You can then use the (P(initial))(V(initial)) = (P(final))(V(final)) You can do this because of the factors that are remaining constant. This will give you partial pressure of gas A. All partial pressures are additive. I think. It's been a few years . I might be wrong. There might be a simpler way then that too..








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Old 26-10-11, 01:48 AM   #10
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Default Re: Chemistry

Quote:
Originally Posted by hippiehobo View Post
i think you just use the volumes at one atmosphere and then combine them
add them all together and there is 2.5 times as much in on container, so 2.5 atmospheres
maybe?
i'm not sure though
That's it. Thank you so much!








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