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21 December, 20:18

The electrolysis of water forms H2 and O2.

2H2O → 2H2 + O2

What is the percent yield of Oz if 10.2 g of Oz is produced from the decomposition of 17.0 g of H20?

Actual yield

Use %Yield = =

Theoretical yield To

15.1%

33.8%

60.1%

67.6%

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Answers (1)
  1. 21 December, 23:07
    0
    67.5% ≅ 67.6%

    Explanation:

    Given dа ta:

    Mass of water = 17.0 g

    Mass of oxygen produced (actual yield) = 10.2 g

    Percent yield of oxygen = ?

    Solution:

    Chemical equation:

    2H₂O → 2H₂ + O₂

    Number of moles of water:

    Number of moles = mass / molar mass

    Number of moles = 17.0 g / 18.016 g/mol

    Number of moles = 0.944 mol

    Now we will compare the moles of oxygen with water to know the theoretical yield of oxygen.

    H₂O : O₂

    2 : 1

    0.944 : 1/2*0.944 = 0.472 mol

    Mass of oxygen:

    Mass = number of moles * molar mass

    Mass = 0.472 mol * 32 g/mol

    Mass = 15.104 g

    Percent yield:

    Percent yield = [Actual yield / theoretical yield] * 100

    Percent yield = [ 10.2 g / 15.104 g] * 100

    Percent yield = 0.675 * 100

    Percent yield = 67.5%
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