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: O [A] = 6.0 and [B] = 0.6 O [A] = 3.0 and [B] = 0.6 O [A] = 4.5 and [B] = 0.6 [A] = 1.5 and [B] = 1.2 O [A] = 3.0 and [B] = 1.8 [A] = 1.5 and [B] = 1.8 O [A] = 3.0 and [B] = 1.2 O [A] = 7.5 and [B] = 0.6 Experiment [A] (M) [B] (M) Rate (M/s) 1 2 Rate = K[A][B][C] Rate = K[A][C] Rate = k[A]² [C] O Rate = K[A][C]² Rate = k[A]²[C]² Rate = k[A]³ [C] O Rate = K[A][C]³ 1.5 3.0 (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]* [B]Y? Choose all correct possibilities. 0.6 0.6 (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. (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
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: O [A] = 6.0 and [B] = 0.6 O [A] = 3.0 and [B] = 0.6 O [A] = 4.5 and [B] = 0.6 [A] = 1.5 and [B] = 1.2 O [A] = 3.0 and [B] = 1.8 [A] = 1.5 and [B] = 1.8 O [A] = 3.0 and [B] = 1.2 O [A] = 7.5 and [B] = 0.6 Experiment [A] (M) [B] (M) Rate (M/s) 1 2 Rate = K[A][B][C] Rate = K[A][C] Rate = k[A]² [C] O Rate = K[A][C]² Rate = k[A]²[C]² Rate = k[A]³ [C] O Rate = K[A][C]³ 1.5 3.0 (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]* [B]Y? Choose all correct possibilities. 0.6 0.6 (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. (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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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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Chapter1: Chemical Foundations
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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![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:
O [A] = 6.0 and [B] = 0.6
O [A] = 3.0 and [B] = 0.6
O [A] = 4.5 and [B] = 0.6
[A] = 1.5 and [B] = 1.2
O [A] = 3.0 and [B] = 1.8
[A] = 1.5 and [B] = 1.8
O [A] = 3.0 and [B] = 1.2
O [A] = 7.5 and [B] = 0.6
Rate = K[A][B][C]
Rate = K[A][C]
Experiment [A] (M) [B] (M) Rate (M/s)
(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]* [B]Y? Choose all correct possibilities.
k[A]² [C]
O Rate = K[A][C]²
Rate = k[A]²[C]²
Rate =
k[A]³ [C]
O Rate = K[A][C]³
1
2
Rate =
1.5
3.0
(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.
0.6
0.6
(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](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F86624ab7-da2a-4a5b-91b8-0bf4ad8ab366%2Fcb16c7b8-6b02-4196-b8c1-0db2d359e656%2Fe6b2mx4_processed.png&w=3840&q=75)
Transcribed Image Text: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:
O [A] = 6.0 and [B] = 0.6
O [A] = 3.0 and [B] = 0.6
O [A] = 4.5 and [B] = 0.6
[A] = 1.5 and [B] = 1.2
O [A] = 3.0 and [B] = 1.8
[A] = 1.5 and [B] = 1.8
O [A] = 3.0 and [B] = 1.2
O [A] = 7.5 and [B] = 0.6
Rate = K[A][B][C]
Rate = K[A][C]
Experiment [A] (M) [B] (M) Rate (M/s)
(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]* [B]Y? Choose all correct possibilities.
k[A]² [C]
O Rate = K[A][C]²
Rate = k[A]²[C]²
Rate =
k[A]³ [C]
O Rate = K[A][C]³
1
2
Rate =
1.5
3.0
(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.
0.6
0.6
(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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