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How much ammonia is produced if 1.80 m3 of hydrogen reacts with 0.5m3 of nitrogen? Also state which reagent is in excess and by how much?
Question is related to the Haber process. Please can anyone answer this for me by 02 July 2010.
With all equations.

  • Chemistry -

    Yes and no. We help do homework but we don't do it for you. Here is the way you go about solving the question. Most of the limiting reagent problems are done this way.
    1. Write and balance the equation.
    N2 + 3H2 ==> 2NH3

    2. When the equation is all gases, one may take a shortcut and NOT convert to moles.
    a. Using the coefficients in the balanced equation, convert volume of N2 to volume of NH3.
    1.8 m^3 H2 x (2 moles NH3/3 moles H2) = 1.8 x (2/3) = ?? m^3 NH3 from H2.

    2b. Do the same for 0.5 m^3 N2.

    2c. It is likely that the volume of NH3 produced according to 2a and 2b will not be the same which means one of them is wrong. The correct answer in limiting reagent problems is ALWAYS the smaller value and the reagent producing that value is the limiting reagent.

    2d. Now that you know how much NH3 is produced and you have determined the limiting reagent, you turn attention to how much of the "other" reagent was used since you know ALL of the limiting reagent was used.
    Same procedure. Use the coefficients to convert volume of the limiting reagent to volume of the "other" reagent. That will tell you how much was used and the difference between the initial value and the amount used will tell you how much is left. Post your work if you get stuck.

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