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 2.0 1.8 2 4.0 1.8 (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] = 4.0 and [B] = 3.6[A] = 4.0 and [B] = 1.8[A] = 2.0 and [B] = 3.6[A] = 4.0 and [B] = 5.4[A] = 10.0 and [B] = 1.8[A] = 8.0 and [B] = 1.8[A] = 6.0 and [B] = 1.8[A] = 2.0 and [B] = 5.4 (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 tripling the concentration of C increases the rate by a factor of 27. 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.

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter12: Chemical Kinetics

Section: Chapter Questions

Problem 3RQ: One experimental procedure that can be used to determine the rate law of a reaction is the method of...

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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)


1	2.0	1.8
2	4.0	1.8

(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] = 4.0 and [B] = 3.6[A] = 4.0 and [B] = 1.8[A] = 2.0 and [B] = 3.6[A] = 4.0 and [B] = 5.4[A] = 10.0 and [B] = 1.8[A] = 8.0 and [B] = 1.8[A] = 6.0 and [B] = 1.8[A] = 2.0 and [B] = 5.4

(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 tripling the concentration of C increases the rate by a factor of 27. 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.

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