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9 May, 17:49

The rate constant is found to be 3.9 x 10-5 M-1 s-1. Calculate the rate of formation of ozone when the concentration of oxygen atoms is 3.0 x 10-14 molar and the concentration of diatomic oxygen is 1.3 x 10-14 molar.

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  1. 9 May, 18:37
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    The answer is 1.5 X 10 ^32 M/s.

    Determine the Chemical reaction:

    O + O₂ → O₃

    Note:

    The Ozone is formed when an oxygen atom collides with a molecule of oxygen.

    Given:

    k = 3.9 x 10-5 M-1 s-1

    Solution:

    c (O) = 3.0 x 10⁻¹⁴ M

    c (O₂) = 1.3 x 10⁻¹⁴ M

    Required:

    Find the rate of formation

    rate of formation = k·c (O) ·c (O₂)

    rate of formation = (3.9 x 10⁻⁵ M⁻¹·s⁻¹) (1.3 x 10⁻¹⁴ M) (3.0 x 10⁻¹⁴ M)

    rate of formation of ozone = 1.5 x 10⁻³² M/s
  2. 9 May, 20:29
    0
    Answer: 1.5x10⁻³² M/s

    Explanation:

    1) The ozone is formed when oxygen atoms (O) react with oxygen diatomic molecules (O₂)

    2) The chemical equation for the formation of ozone is:

    O + O₂ → O₃

    3) The rate of the formation is:

    rate = k[O][O2]

    4) You are given the three values k,[O] and [O2], so just plug in and calculate:

    rate = 3.9·10⁻⁵ M⁻¹·s⁻¹ · 1.3·10⁻¹⁴ M · 3.0·10⁻¹⁴ M. = 1.5x10⁻³² M/s
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