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Chemistry

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Ammonia (NH3) is formed industrially by reacting nitrogen and hydrogen gases. How many liters of ammonia gas can be formed from 13.7L of hydrogen gas at 93.0 degrees Celsius and a pressure of 2.25atm?

  • Chemistry - ,

    now if i wrote out the equation..
    N2 + H2 ==> NH3
    then balanced it..
    3N2 + H2 ==> 2NH3
    could the numbers given possibly just be extra information that is unneeded, and the volume of ammonia simply be 2 * 22.42 because its at STP?
    i really would appreciate some help here..

  • Chemistry - ,

    ok i wrote the other coefficients wrong wow its getting too late for this

  • Chemistry - ,

    Write and balance the equation.
    N2 + 3H2 ==> 2NH3.
    Use PV = nRT to determine n (# mols) for H2 at the conditions listed.
    Convert mols H2 to mols NH3 using the coefficients in the balanced equation.
    I assume the question is asking for volume of NH3 produced at the non-standard conditions. Use PV = nRT to convert mols to volume at the non-standard conditions. Post your work if you get stuck.

  • Chemistry - ,

    Erm.. ok..
    PV = nRT
    (2.25)(13.7) = n(.08206)(366.15)
    n = 1.026

    1.026molH2 * 2molNH3/3molH2 = .684molNH3
    PV=nRT
    (?)(?)=(.684)(.08206)(?)

  • Chemistry - ,

    Ohh, nevermind, your saying I should use the same values I used before for P and T ok..
    what I got was 9.13L NH3
    thank you so much for your help!

  • Chemistry - ,

    9.13 L is correct. By the way, there is a much easier way to do this that I forgot to post after doing it the hard way. But th long way ALWAYS works and this short cut works only in circumstances where all of the materials are gaseous at the conditions listed AND we want the final conditions at th same P and T as the initial conditions. When all are gases, we can cut out the mole step and simply use volumes.
    13.7 L x (2 mols NH3/3 mols H2) = 13.7 x 2/3 = 9.13 L. Quick, huh?

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