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: (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, Ratek [A] [B]"? Choose all correct possibilities. [A]1.3 and [B] 0.6 O [A] 3.9 and [B] -0.3 O [A] 2.6 and [B] -0.3 O [A] 2.6 and [B] -0.9 O [A] 6.5 and [B] -0.3 [A] 5.2 and [B] = 0.3 O [A] 2.6 and [B] -0.6 O [A] 1.3 and [8] = 0.9 Experiment [A] (M) [B] (M) Rate (M/s) 22 2.6 (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. O Rate k[A][B][C] O Rate k[A][C] Rate = K[A]²[C] O Rate = K[A][C]2 O Rate k[A]2 [C]² O Rate = K[A] [C] O 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 2
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: (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, Ratek [A] [B]"? Choose all correct possibilities. [A]1.3 and [B] 0.6 O [A] 3.9 and [B] -0.3 O [A] 2.6 and [B] -0.3 O [A] 2.6 and [B] -0.9 O [A] 6.5 and [B] -0.3 [A] 5.2 and [B] = 0.3 O [A] 2.6 and [B] -0.6 O [A] 1.3 and [8] = 0.9 Experiment [A] (M) [B] (M) Rate (M/s) 22 2.6 (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. O Rate k[A][B][C] O Rate k[A][C] Rate = K[A]²[C] O Rate = K[A][C]2 O Rate k[A]2 [C]² O Rate = K[A] [C] O 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 2
Chemistry: The Molecular Science
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ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter11: Chemical Kinetics: Rates Of Reactions
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part "a" and "c"
![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] = 1.3 and [B] = 0.6
O [A] = 3.9 and [B] 0.3
O [A] = 2.6 and [B] = 0.3
O [A] = 2.6 and [B] = 0.9
O [A] = 6.5 and [B] = 0.3
[A] = 5.2 and [B] = 0.3
O [A] = 2.6 and [B] = 0.6
O [A] = 1.3 and [B] = 0.9
X
(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.
O Rate = k[A][B][C]
O Rate = K[A][C]
Rate = k[A]² [c]
O Rate = K[A][C]²
O Rate = K[A]² [C]²
O Rate = K[A]³ [C]
O Rate = K[A][C]³
Experiment [A] (M) [B] (M) Rate (M/s)
1
2
The rate will be the original rate multiplied by a factor of 2
1.3
2.6
(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.
X.
(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)?
0.3
0.3](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fe19901ac-7755-4e8b-9a1f-9a115e123c4b%2F58d7ed38-7c98-42fb-ae2d-b3626c215d59%2Fa69wgpr_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] = 1.3 and [B] = 0.6
O [A] = 3.9 and [B] 0.3
O [A] = 2.6 and [B] = 0.3
O [A] = 2.6 and [B] = 0.9
O [A] = 6.5 and [B] = 0.3
[A] = 5.2 and [B] = 0.3
O [A] = 2.6 and [B] = 0.6
O [A] = 1.3 and [B] = 0.9
X
(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.
O Rate = k[A][B][C]
O Rate = K[A][C]
Rate = k[A]² [c]
O Rate = K[A][C]²
O Rate = K[A]² [C]²
O Rate = K[A]³ [C]
O Rate = K[A][C]³
Experiment [A] (M) [B] (M) Rate (M/s)
1
2
The rate will be the original rate multiplied by a factor of 2
1.3
2.6
(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.
X.
(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)?
0.3
0.3
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