Calculate the reaction order for each species m and n. Report two values for each reaction order, the exact determine value and the nearest integer value.
Calculate the reaction order for each species m and n. Report two values for each reaction order, the exact determine value and the nearest integer value.
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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Calculate the reaction order for each species m and n. Report two values for each reaction order, the exact determine value and the nearest integer value.
![[Oxalic acid]stock = 0.755 M; [KMnO4] = 0.130 M
[Oxalic
[KMNO4]
Average Reaction
time
(sec)
Trial acid]
Rate
(M/s)
M
Trial-
0.3146 0.0108
1
3.85 *
280.79
|10-5
Trial-
0.6292 0.0108
|6.04 *
178.78
10-5
Trial-
0.3146 0.0216
3.81 *
564.22
|10-5
3
Reaction Rate =[MnO4]/ Av. time](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F4d4f45f0-6f0b-4cb6-9f2e-05d769dd18ce%2F47d1378d-ee9a-47bb-9315-22dfb829fef9%2Fg98xoho_processed.jpeg&w=3840&q=75)
Transcribed Image Text:[Oxalic acid]stock = 0.755 M; [KMnO4] = 0.130 M
[Oxalic
[KMNO4]
Average Reaction
time
(sec)
Trial acid]
Rate
(M/s)
M
Trial-
0.3146 0.0108
1
3.85 *
280.79
|10-5
Trial-
0.6292 0.0108
|6.04 *
178.78
10-5
Trial-
0.3146 0.0216
3.81 *
564.22
|10-5
3
Reaction Rate =[MnO4]/ Av. time
![Determination of the Rate Law for the Oxidation of Oxalic Acid
by Permanganate
To learn about the Kinetics of Chemical Reactions.
To learn about the Reaction Rate.
To learn about the Factors Affecting the Chemical Reaction Rate.
To learn about Rate Laws.
In this laboratory exercise we will determine the Rate Law for the reaction between
Permanganate (MnO4²) and Oxalic Acid (H2C204).
3 H2C2O4(aq) + 2 MnO4 (aq)
To sten
6 CO2(g) + 2 MnO2(s) + 2 OH (aq) + 2 H2O
bniw
clear sol'n
purple sol'n
yellow colloid
(Eq. 1)
It is expected the Rate Law for this reaction will have a simple form:
k [H2C2O4]™ [Mn04]"
(Eq. 2)
Rate =](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F4d4f45f0-6f0b-4cb6-9f2e-05d769dd18ce%2F47d1378d-ee9a-47bb-9315-22dfb829fef9%2Fhgwytq_processed.jpeg&w=3840&q=75)
Transcribed Image Text:Determination of the Rate Law for the Oxidation of Oxalic Acid
by Permanganate
To learn about the Kinetics of Chemical Reactions.
To learn about the Reaction Rate.
To learn about the Factors Affecting the Chemical Reaction Rate.
To learn about Rate Laws.
In this laboratory exercise we will determine the Rate Law for the reaction between
Permanganate (MnO4²) and Oxalic Acid (H2C204).
3 H2C2O4(aq) + 2 MnO4 (aq)
To sten
6 CO2(g) + 2 MnO2(s) + 2 OH (aq) + 2 H2O
bniw
clear sol'n
purple sol'n
yellow colloid
(Eq. 1)
It is expected the Rate Law for this reaction will have a simple form:
k [H2C2O4]™ [Mn04]"
(Eq. 2)
Rate =
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