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One of the intermediates in the synthesis of glycine from ammonia, carbondioxide and methane is aminoacetonitrile C2H4N2. The balanced chemical equation is 3CH4+5 CO2 + 8NH3 - --> 4C2H4N2 + 10H2O. How much C2H4N2 could be expected from the reaction of 13.2 g CO2, 2.18 g NH3 and 17.0 g CH4

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  1. Today, 19:17
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    mass of C₂H₄N₂ = 3.472 g

    Explanation:

    We have the following chemical reaction:

    3 CH₄ + 5 CO₂ + 8 NH₃ → 4 C₂H₄N₂ + 10 H₂O

    Using the masses given by the problem we calculate the number of moles for each reactant:

    number of moles = mass / molecular weight

    number of moles of CO₂ = 13.2 / 44 = 0.3 moles

    number of moles of NH₃ = 2.18 / 17 = 0.13 moles

    number of moles of CH₄ = 17 / 16 = 1.06 moles

    We can see that the limiting reactant is ammonia NH₃. Now we can devise the following reasoning:

    if 8 moles of NH₃ produces 4 moles of C₂H₄N₂

    then 0.13 moles of NH₃ produces X moles of C₂H₄N₂

    X = (0.13 * 4) / 8 = 0.062 moles of C₂H₄N₂

    mass of C₂H₄N₂ = number of moles * molecular weight

    mass of C₂H₄N₂ = 0.062 * 56 = 3.472 g
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