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chem

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a) Calculate the pressure exerted by 0.5160 mol N2 in a 1.0000 L container at 24.6°C using the ideal gas law.
atm


(b) Calculate the pressure exerted by 0.5160 mol N2 in a 1.0000 L container at 24.6°C using the van der Waals equation.
atm


(c) Compare the results. (Write the percentage difference between the results, based on the higher value result.)
%

  • chem - ,

    Surely you know how to do these. Perhaps you just want to know what answer I get but I don't have the time to work these things unless I have a reason. If you truly don't understand them, explain what kind of problem you are having.

  • chem - ,

    so i plugged int he information that i have from the question... i am using an electronic based hmwk. it says that the answers that i have gotten are wrong... here is what i have come up with....

    with using PV=nRT
    i got a pressure of 12.6012 atm...

    with using the van der w.
    i got apressure of 12.2816 rounded

    am i even close?

  • chem - ,

    I have 12.61 atm. Is the T given as 24.6 or 24.60? If 24.6 then you are allowed 3 sifnificant figures and the answer would be 12.6 atm. If 24.60, then 12.61 atm would be the answer.

  • chem - ,

    For the van der Waals question I have 12.75 but I think only three s.f. are allowed so that would round to 12.7. Check my arithmetic.

  • chem - ,

    or 12.8 if we round to the nearest whole even number.

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