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AB(g) → A(g) + B(g)

Rate = k[AB]^2

k = 0.2L/mol∙S

How long will it take for [AB] to reach 1/3 (one third) of its initial concentration of 1.50M? What is [AB] after 10.0 seconds?

2nd order overall reaction so:

part A

1/[A] - 1/[A]o = (k)(t)

1/0.5 - 1/1.50 = (0.2)(t)

6.667 = t

part B

1/[A] - 1/1.5 = (0.2)(10 s)

[A] = 0.375

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# Rate law seconds and concentration

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