Determine the rate law and rate constant for the following reaction. Don't forget the units. Some of the numbers are blurry. (The concentrations for H+ are x 10-5 and the rates are x 10-7 with the last value being x10-8) 10,(aq) + 81 (aq) + 6 H*(aq) → 3 15 (aq) + 2 H₂O(aq) Initial Rate (M/s) 2.70 x 10 5.40 x 10 6.07 x 10 6.75 x 10 Trial 1 2 3 4 [103] 0.0050 0.0100 0.0050 0.0050 0.030 0.030 0.045 0.030 [H*]o 2.0 x 10 2.0 x 105 2.0 x 10 1.0 x 10
Determine the rate law and rate constant for the following reaction. Don't forget the units. Some of the numbers are blurry. (The concentrations for H+ are x 10-5 and the rates are x 10-7 with the last value being x10-8) 10,(aq) + 81 (aq) + 6 H*(aq) → 3 15 (aq) + 2 H₂O(aq) Initial Rate (M/s) 2.70 x 10 5.40 x 10 6.07 x 10 6.75 x 10 Trial 1 2 3 4 [103] 0.0050 0.0100 0.0050 0.0050 0.030 0.030 0.045 0.030 [H*]o 2.0 x 10 2.0 x 105 2.0 x 10 1.0 x 10
Introduction to General, Organic and Biochemistry
11th Edition
ISBN:9781285869759
Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres
Publisher:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres
Chapter7: Reaction Rates And Chemical Equilibrium
Section: Chapter Questions
Problem 7.10P: 7-10 The rate of disappearance of HCI was measured for the following reaction: The initial...
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![Determine the rate law and rate constant for the following reaction. Don't forget the
units. Some of the numbers are blurry. (The concentrations for H* are x 10-5 and
the rates are x 10-7 with the last value being x10-8)
10, (aq) + 81(aq) + 6 H*(aq) → 31, (aq) + 2 H₂O(aq)
Initial Rate (M/s)
2.70 x 10
5.40 x 10
6.07 x 10
6.75 x 10
Trial [103]
1
0.0050
2
0.0100
3
0.0050
4
0.0050
[I]
0.030
0.030
0.045
0.030
[H*].
2.0 x 10
2.0 x 10
2.0 x 10
1.0 x 10](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F21ed1cfb-364f-46d5-bbe5-45039b5aabf3%2F82b83b76-3d5d-4b62-ad20-1b5aba4e851a%2Feq83i8a_processed.png&w=3840&q=75)
Transcribed Image Text:Determine the rate law and rate constant for the following reaction. Don't forget the
units. Some of the numbers are blurry. (The concentrations for H* are x 10-5 and
the rates are x 10-7 with the last value being x10-8)
10, (aq) + 81(aq) + 6 H*(aq) → 31, (aq) + 2 H₂O(aq)
Initial Rate (M/s)
2.70 x 10
5.40 x 10
6.07 x 10
6.75 x 10
Trial [103]
1
0.0050
2
0.0100
3
0.0050
4
0.0050
[I]
0.030
0.030
0.045
0.030
[H*].
2.0 x 10
2.0 x 10
2.0 x 10
1.0 x 10
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