chemistry! URGENT!!!

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A gaseous mixture of O2 and N2 contains 30.8 % nitrogen by mass. What is the partial pressure of oxygen in the mixture if the total pressure is 365 mmHg?

  • chemistry! URGENT!!! -

    First you have to find the moles of O2 and N2. To do this you must assume that this is a 100g sample. Therefore, 30.8g of nitrogen. Now you can find the moles of nitrogen by dividing this mass by nitrogen's molar mass:

    30.8g/(14.01g/mol x 2) = 1.10moles N2

    Next you can find the moles of oxygen by subracting 100 by the mass of nitrogen.

    100-30.8g N2 = 69.2g O2

    Now you can find the moles of oxygen:

    69.2g/(16.0g/mol x 2) = 2.16moles O2

    You can find the mole fraction of oxygen by using the equation :

    O2=moles of component/total moles in mixture
    =2.16moles/(2.16moles + 1.10moles)
    =0.659

    Lastly, you can find your partial pressure by multiplying the mole fraction of oxygen that you just found by the total pressure given in the question.

    P1=O × Ptotal
    =0.659 x 365mmHg
    =240mmHg

    Hope this helps!! :)

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