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4 July, 10:07

Nitrogen dioxide undergoes thermal decomposition according to the second-order reaction 2 NO2 (g) → 2 NO (g) + O2 (g). When 0.700 M NO2 is allowed to react for 90.0 seconds, its concentration falls to 0.0463 M. What is the rate constant for the reaction?

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  1. 4 July, 13:25
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    K = 0.2241 M-1 s-1

    Explanation:

    2 NO2 (g) → 2NO (g) + O2 (g) - ra = K * (Ca) ∧α = - δCa/δt [=] M/s

    ∴ a: NO2

    ∴ α = 2 ... second order

    ⇒ - δCa/δt = K Ca²

    ⇒ - ∫δCa/Ca² = K*∫δt

    ⇒ [ 1/Ca - 1/Cao ] = K*t

    ∴ Ca = 0.0463 M

    ∴ Cao = 0.700 M

    ∴ t = 90.0 s

    rate constant (K):

    ⇒ - [ 1/0.0463 - 1/0.700 ] = K * (90.0 s)

    ⇒ 20.1697 M-1 = K * (90.0 s)

    ⇒ K = 0.2241 M-1 s-1
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