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19 January, 00:45

3. A 0.500 g sample of nitrogen gas combines with 1.140 g of oxygen gas to form NO2. If the atomic mass of oxygen is 16.000, calculate the atomic mass of nitrogen from this data.

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  1. 19 January, 01:05
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    Answer;

    = 18.24

    Explanation;

    The ratio of N and O in the formula NO2 IS 1:2

    Mass of nitrogen gas is 0.500 g

    Moles of nitrogen will be;

    = 0.500/16 = 0.03125 moles

    Therefore;

    The moles of Oxygen from the ratio will be;

    = 0.03125 * 2 = 0.0625 moles

    But; 0.0625 moles is equal to 1.140 g of Oxygen

    The atomic number (mass in 1 mole) will be;

    = 1.140 / 0.0625

    = 18.24

    Thus the atomic number of Oxygen from the data is 18.24
  2. 19 January, 01:12
    0
    The balanced chemical equation for the given reaction is:

    N₂ + 2O₂ → 2NO₂

    According to the given balanced equation, 2 moles of O₂ combines with 1 mole of O₂

    Given, Mass of O₂ = 1.140 g

    Atomic mass of O = 16 amu

    Molar mass of O₂ = 16 x 2 = 32 g/mol

    Now to calculate the moles of N₂:

    1.14 g of O₂ x (1 mole of O₂ / 32 g of O₂) x (1 mol of N₂ / 2 mol O₂) = 0.0178 mol of N₂

    Molar mass = mass / moles

    Given, Mass of N₂ = 0.500 g

    Molar mass of N₂ = 0.500 g / 0.0178 mol = 28 g/mol

    Atomic mass of N = 28/2 = 14 amu

    Therefore, the atomic mass of N is 14 amu
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