14.2 Rate Laws

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    rate laws
    Rate Orders
    Zero Order A ➔ B Rate = k
    1st Order M ➔ N Rate = k[M]
    2nd Order X ➔ Y Rate = k[X]2

    Rate laws must be determined from experimental data
    2NO(g) + Cl2(g) ⇌ 2NOCl(g)
    The following data were obtained for the reaction above:

    [NO]0 (M) [Cl2]0 (M) Initial Rate (M/s)
    0.10 0.10 0.18
    0.10 0.20 0.36
    0.20 0.20 1.44

    What is the rate law for this reaction?

    What is the rate constant?