by Inzaghi on February 24th, 2007

Inzaghi

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A gas cylinder contains 6400g of Oxygen at a pressure of 5atms. an EXACTLY similar cylinder contains 4200g of Nitrogen at the same temperature. What is the pressure on the N. (Molecular weights;Oxygen=32,Nitrogen= 23;Assume both behaves as a perfect gas)

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Answers. 2 helpful answers below.

  • by CannedHam on February 25th, 2007

    CannedHam

    Do your own damn homework, kid.

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  • by Quirkie on February 25th, 2007

    Quirkie

    Yeah so these might be homework questions, but answerbag can still help. A good answer might help you do these questions in the future, not just this homework.

    For this question need to use the gas laws. Assuming you aren't forced to use the individual laws, (and I can only remember Boyle's law), all you need is the equation:

    PV = nRT
    where R is a constant.

    Here V and T are constant so we can rearrange to get:
    P / n = some constant for this question.

    n is mass in mols, which is mass in grams divided by molecular weight.

    For oxygen it will be 6400/32 = 200
    For nitrogen it is 4200/28 = 150
    (Yes 28, 23 is wrong).

    So (5 atms / 200) = (x atms / 150)
    x = 3.75 atms.

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