(d) Determine the initial rate of change of [A] in Experiment 3. (note that the initial rates are with respect to [C]) (e) Identify which of the reaction mechanisms represented below is consistent with the rate law developed in part (b). Justify your choice. 1. A+BOC+M Fast Justify M+ALD Slow 2. B2M Fast equilibrium M+ALC+X Slow A+ XL D Fast Fast equilibrium Slow 3. A+B2M M+ALC+X XL D Fast (f) For experiment 2, calculate the concentration of B remaining when exactly one-half of the original amount of A had been consumed.
(d) Determine the initial rate of change of [A] in Experiment 3. (note that the initial rates are with respect to [C]) (e) Identify which of the reaction mechanisms represented below is consistent with the rate law developed in part (b). Justify your choice. 1. A+BOC+M Fast Justify M+ALD Slow 2. B2M Fast equilibrium M+ALC+X Slow A+ XL D Fast Fast equilibrium Slow 3. A+B2M M+ALC+X XL D Fast (f) For experiment 2, calculate the concentration of B remaining when exactly one-half of the original amount of A had been consumed.
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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Can you help me with D, E, and F?
![11.
2A+BOC+ D
The following results were obtained when the reaction represented above was studied at 25°C.
Experiment #
Initial, [A].
Initial, [B].
Initial Rate of Formation of C
(mol L' min')
1
0.25
0.75
4.3 x 104
0.75
0.75
1.3 x 103
3
1.50
1.50
5.3 x 103
4
1.75
?
8.0 x 103
(a) Determine the order of the reaction with respect to A and to B. Justifv vour answer. (trickier logic here, I think)
1.3X10:3=C0.75] [0,75]* S.3xiD-SD)" (1 SD)M
1.3X10-3 Co.75) [0.75]
order w/ nespect to A: First
order w/ nespect to BiArSt
3-B]"
2=6)" y=1
Write the rate law for the reaction: ate=L[A]B]
ソー」
(b)
%3D
(c)
Calculate the value of the rate constant, specifying units.
4.3X10M molL"'min
0.25moll--(0.75) moll"
(d) Determine the initial rate of change of [A] in Experiment 3. (note that the initial rates are with respect to [C])
- 2.79 V1D3 mol'Lmin' (2.29x 103M min-h
2.29 103M min
(e) Identify which of the reaction mechanisms represented below is consistent with the rate law developed in
part (b). Justify your choice.
1.
A+B C+ M
Fast
Justify
M+ALD
Slow
2.
B2M
Fast equilibrium
M+ALC+X
Slow
A+XL D
Fast
3.
A+B2M
Fast equilibrium
M+ALC+X
Slow
XL D
Fast
(f) For experiment 2, calculate the concentration of B remaining when exactly one-half of the original amount of A
had been consumed.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F9b1d6994-83c0-472b-a60c-05f27149766f%2Fac71bfa1-e36a-4e79-baf9-9c126ee38575%2Fvh3ta9k_processed.jpeg&w=3840&q=75)
Transcribed Image Text:11.
2A+BOC+ D
The following results were obtained when the reaction represented above was studied at 25°C.
Experiment #
Initial, [A].
Initial, [B].
Initial Rate of Formation of C
(mol L' min')
1
0.25
0.75
4.3 x 104
0.75
0.75
1.3 x 103
3
1.50
1.50
5.3 x 103
4
1.75
?
8.0 x 103
(a) Determine the order of the reaction with respect to A and to B. Justifv vour answer. (trickier logic here, I think)
1.3X10:3=C0.75] [0,75]* S.3xiD-SD)" (1 SD)M
1.3X10-3 Co.75) [0.75]
order w/ nespect to A: First
order w/ nespect to BiArSt
3-B]"
2=6)" y=1
Write the rate law for the reaction: ate=L[A]B]
ソー」
(b)
%3D
(c)
Calculate the value of the rate constant, specifying units.
4.3X10M molL"'min
0.25moll--(0.75) moll"
(d) Determine the initial rate of change of [A] in Experiment 3. (note that the initial rates are with respect to [C])
- 2.79 V1D3 mol'Lmin' (2.29x 103M min-h
2.29 103M min
(e) Identify which of the reaction mechanisms represented below is consistent with the rate law developed in
part (b). Justify your choice.
1.
A+B C+ M
Fast
Justify
M+ALD
Slow
2.
B2M
Fast equilibrium
M+ALC+X
Slow
A+XL D
Fast
3.
A+B2M
Fast equilibrium
M+ALC+X
Slow
XL D
Fast
(f) For experiment 2, calculate the concentration of B remaining when exactly one-half of the original amount of A
had been consumed.
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