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1 July, 03:41

He rate law for the reaction 3 a c is rate = 4.36 ✕ 10-2 l mol-1 hr-1[a]2 what is the half-life for the reaction if the initial concentration of a is 0.250 m?

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  1. 1 July, 03:45
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    d[C] dt =.0436[A ]2 d[C] dt =.0436[A ]2

    d[A] dt = - 3 d[C] dt d[A] dt = - 3 d[C] dt

    d[A] dt = -.1308[A ]2 d[A] dt = -.1308[A ]2

    - 1 [A ]2 d[A]=.1308dt - 1 [A ]2 d[A]=.1308dt

    1 [A] =.1308t+C 1 [A] =.1308t+C

    [A] = 1.1308t+C [A] = 1.1308t+C

    .250 = 1C. 250 = 1C

    C=4 C=4

    .125 = 1.1308t+4.125 = 1.1308t+4

    t = (1.125 - 4) ∗ 1.1308 = 30.58 t = (1.125 - 4) ∗ 1.1308 = 30.58

    Assuming I did my math right, looks fine to me, it should be about 30 hours and 30 minutes.
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