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	1.9	0.1
2	3.8	0.1

(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] = 3.8 and [B] = 0.2

[A] = 5.7 and [B] = 0.1

[A] = 3.8 and [B] = 0.1

[A] = 1.9 and [B] = 0.2

[A] = 7.6 and [B] = 0.1

[A] = 9.5 and [B] = 0.1

[A] = 3.8 and [B] = 0.3

[A] = 1.9 and [B] = 0.3 (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 4, doubling the concentration of B has no effect on the rate, and tripling the concentration of C increases the rate by a factor of 9. 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]²Rate = k[A]² [C]²Rate = 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 ...