Question

You and your lab partner are studying the rate of a reaction, A + B --> C. You make measurements of the initial rate under the following conditions:

Experiment [A] (M) [B] (M) Rate (M/s)
1 0.2 1.9
2 0.4 1.9



(a) Which of the following reactant concentrations could you use for experiment 3 in order to determine the rate law, assuming that the rate law is of the form, Rate = k [A]x [B]y? Choose all correct possibilities.

[A] = 0.6 and [B] = 1.9

[A] = 0.4 and [B] = 3.8

[A] = 1.0 and [B] = 1.9

[A] = 0.4 and [B] = 5.7

[A] = 0.2 and [B] = 3.8

[A] = 0.4 and [B] = 1.9

[A] = 0.2 and [B] = 5.7

[A] = 0.8 and [B] = 1.9




(b) For a reaction of the form, A + B + C --> Products, the following observations are made: doubling the concentration of A increases the rate by a factor of 2, doubling the concentration of B has no effect on the rate, and doubling the concentration of C increases the rate by a factor of 2. Select the correct rate law for this reaction from the choices below.

Rate = k[A][B][C]

Rate = k[A][C]   

Rate = k[A]2 [C]

Rate = k[A][C]2

Rate = k[A]2 [C]2

Rate = k[A]3 [C]

Rate = k[A][C]3



(c) By what factor will the rate of the reaction described in part (b) above change if the concentrations of A, B, and C are all halved (reduced by a factor of 2)?

The rate will be the original rate multiplied by a factor of ______.

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