#2A(g) + B(g) -> C(g)#. Rate = #k[A]^2[B]#. At the beginning of one trial of this reaction, [A] = 4.0 M and [B] = 1.0 M. The observed rate was 0.048 #"mol"*"L"^(-1)*"s"^(-1)#. What is the value of the rate constant for this reaction closest to?

1 Answer
Ernest Z.
Jan 3, 2017

The value of the rate constant is #"0.030 L"^2"mol"^"-2""s"^"-1"#.

Explanation:

The rate law is

#"rate" = k["A"]^2["B"]#

∴ #k = "rate"/(["A"]^2["B"]) = (0.048 color(red)(cancel(color(black)("mol·L"^"-1")))"s"^"-1")/(("4.0 mol·L"^"-1")^2 × 1.0 color(red)(cancel(color(black)("mol·L"^"-1")))) = "0.0030 L"^2"mol"^"-2""s"^"-1"#

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