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22 August, 05:35

Consider the reaction of Mg3N2 with H2O to form Mg (OH) 2 and NH3. If 4.33 g H2O is reacted with excess Mg3N2 and 6.26 g of Mg (OH) 2 is ultimately isolated, what is the percent yield for the reaction?

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  1. 22 August, 05:58
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    89.34%

    Explanation:

    First, write a balanced reaction.

    Mg3N2 + 6H2O - -> 3Mg (OH) 2 + 2NH3

    Next determine the moles of the known substance, or limiting reagent (H2O)

    n = m/MM

    n (H2O) = 4.33 / (1.008*2) + 16

    n (H2O) = 0.2403

    Use the mole ratio to find the moles of Mg (OH) 2

    0.2403 : 2

    n (Mg (OH) 2) = 0.1202

    Next, find the theoretical mass of Mg (OH) 2 that should have been produced

    m = n * MM

    m = 0.1202 * (24.305 + (16*2) + (1.008 * 2))

    =7.007g

    To find percentage yield, divide the experimental amount by the theoretical amount and multiply by 100.

    6.26 / 7.007 * 100

    =89.34%
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