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Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter11: Chemical Kinetics: Rates Of Reactions

Section11.2: Effect Of Concentration On Reaction Rate

Problem 11.3PSP

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Question

24. 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	1.1	0.8
2	2.2	0.8

(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] = 2.2 and [B] = 1.6

[A] = 2.2 and [B] = 2.4[

A] = 3.3 and [B] = 0.8

[A] = 1.1 and [B] = 2.4

[A] = 5.5 and [B] = 0.8

[A] = 4.4 and [B] = 0.8

[A] = 2.2 and [B] = 0.8

[A] = 1.1 and [B] = 1.6

(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 9, 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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