Answered: Experiment [A] (M) [B] (M) Rate (M/s)…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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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	0.1	0.9
2	0.2	0.9

(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] = 0.2 and [B] = 0.9

[A] = 0.2 and [B] = 1.8

[A] = 0.1 and [B] = 1.8

[A] = 0.4 and [B] = 0.9

[A] = 0.1 and [B] = 2.7

[A] = 0.3 and [B] = 0.9

[A] = 0.5 and [B] = 0.9

[A] = 0.2 and [B] = 2.7

(b) For a reaction of the form, A + B + C --> Products, the following observations are made: tripling the concentration of A increases the rate by a factor of 27, 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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