Ask Question
10 January, 07:45

Determine the rate law and the value of k for the following reaction using the data provided. NO2 (g) + O3 (g) → NO3 (g) + O2 (g) [NO2]i (M) [O3]i (M) Initial Rate0.10 0.33 1.420.10 0.66 2.840.25 0.66 7.10Rate = 430 M-2s-1[NO2]2[O3]Rate = 130 M-2s-1[NO2][O3]2Rate = 1360 M-2.5s-1[NO2]2.5[O3]Rate = 43 M-1s-1[NO2][O3]Rate = 227 M-2.5s-1[NO2][O3]2.5

+4
Answers (1)
  1. 10 January, 08:25
    0
    Rate = 43 M⁻¹s⁻¹[NO₂][O₃]

    Explanation:

    We need to find the reaction order in

    rate = (NO₂) ᵃ (O₃) ᵇ

    given:

    (NO₂) M (O₃) M Rate M/s

    0.10 0.33 1.420 (1)

    0.10 0.66 2.840 (2)

    0.25 0.66 7.10 (3)

    When keeping the NO₂ concentration constant in the first two while doubling the concentration of O₃, the rate doubles. Therefore it is first order with respect to O₃

    Comparing (2) and (3) increasing the concentration of NO₂ by a factor of 2.5 and keeping O₃ constant, increased the rate by a factor of 2.5. Therefore the rate is first order with respect to NO₂

    Then rate law is

    = k (NO₂) (O₃)

    To find k take any of the three and substitute the values to find k:

    1.420 M/s = k (0.10) M x (0.33) M ⇒ k = 43 / Ms

    Then the answer is Rate = 43 M⁻¹s⁻¹[NO₂][O₃]
Know the Answer?
Not Sure About the Answer?
Get an answer to your question ✅ “Determine the rate law and the value of k for the following reaction using the data provided. NO2 (g) + O3 (g) → NO3 (g) + O2 (g) [NO2]i ...” in 📙 Chemistry if there is no answer or all answers are wrong, use a search bar and try to find the answer among similar questions.
Search for Other Answers