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29 May, 12:54

In Haber's process, 30 moles of hydrogen and 30 moles of nitrogen react to make ammonia. If the yield of the product is 50%, what is the mass of nitrogen remaining after the reaction?

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Answers (2)
  1. 29 May, 13:05
    0
    25 moles

    Explanation:

    1 mole of nitrogen reacts with 3 moles of hydrogen to give 2 moles of ammonia. 30 moles of hydrogen will react with 10 moles of nitrogen to give 20 moles of ammonia. As the actual yield is 50%, ammonia formed is 10 moles, the amount of nitrogen reacted is 5 moles, and the amount of hydrogen reacted is 15 moles. The mass of the remaining hydrogen is 15 moles and of the remaining nitrogen is 25 moles.
  2. 29 May, 15:18
    0
    Therewill be produced 170.6 grams NH3, there will remain 25 moles of N2, this is 700 grams

    Explanation:

    Step 1: Data given

    Number of moles hydrogen = 30 moles

    Number of moles nitrogen = 30 moles

    Yield = 50 %

    Molar mass of N2 = 28 g/mol

    Molar mass of H2 = 2.02 g/mol

    Molar mass of NH3 = 17.03 g/mol

    Step 2: The balanced equation

    N2 + 3H2 → 2NH3

    Step 3: Calculate limiting reactant

    For 1 mol of N2, we need 3 moles of H2 to produce 2 moles of NH3

    Hydrogen is the limiting reactant.

    The 30 moles will be completely be consumed.

    N2 is in excess. There will react 30/3 = 10 moles

    There will remain 30 - 10 = 20 moles (this in the case of a 100% yield)

    In a 50 % yield, there will remain 20 + 0,5*10 = 25 moles. there will react 5 moles.

    Step 4: Calculate moles of NH3

    There will be produced, 30 / (3/2) = 20 moles of NH3 (In case of 100% yield)

    For a 50% yield there will be produced, 10 moles of NH3

    Step 5: Calculate the mass of NH3

    Mass of NH3 = mol NH3 * Molar mass NH3

    Mass of NH3 = 20 moles * 17.03

    Mass of NH3 = 340.6 grams = theoretical yield (100% yield)

    Step 6: Calculate actual mass

    50% yield = actual mass / theoretical mass

    actual mass = 0.5 * 340.6

    actual mass = 170.3 grams

    Step 7: The mass of nitrogen remaining

    There remain 20 moles of nitrogen + 50% of 10 moles = 25 moles remain

    Mass of nitrogen = 25 moles * 28 g/mol

    Mass of nitrogen = 700 grams
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