Question 5. You are very familiar with the various clock reactions that make iodine in some form or other. The two you have done in lab use either iodate or iodide as the iodine "source." However, iodate can be used as a test for iodine according to the reaction: 10: (aq) + 5 1"(aq) + 6 H*(aq) → 3 Iz(aq) + 3 H20(1) This reaction was studied at 25 °C with different concentrations of the reactants and the results shown in the Table: Expt [103] mol dm3 1 [1"] mol dm³ [H*] mol dm³ Rate, mol dm³ s³! 0.10 0.010 0.010 0.60 2 0.10 0.040 0.010 2.40 3 0.30 0.010 0.010 5.40 4 0.10 0.010 0.020 2.40 Use these data to determine the order of the reaction with respect to all 3 species. Indicate your reasoning/working in each case. (a) (b) Calculate the rate constant for this reaction at this temperature and give units (c) Discuss the probability of this reaction occurring in a single step. (d) Kinetic studies of reactants are often done under conditions to make them pseudo- first order. Describe what is meant by this term. What reaction conditions would have to be changed to make this study pseudo-first order in l-? The activation energy for this reaction was found to be 84 kJ mol1 at 25 °C. By how must faster would the reaction proceed if the activation energy were lowered bv 10 kJ mol1 (using a suitable catalyst)? (e)
Question 5. You are very familiar with the various clock reactions that make iodine in some form or other. The two you have done in lab use either iodate or iodide as the iodine "source." However, iodate can be used as a test for iodine according to the reaction: 10: (aq) + 5 1"(aq) + 6 H*(aq) → 3 Iz(aq) + 3 H20(1) This reaction was studied at 25 °C with different concentrations of the reactants and the results shown in the Table: Expt [103] mol dm3 1 [1"] mol dm³ [H*] mol dm³ Rate, mol dm³ s³! 0.10 0.010 0.010 0.60 2 0.10 0.040 0.010 2.40 3 0.30 0.010 0.010 5.40 4 0.10 0.010 0.020 2.40 Use these data to determine the order of the reaction with respect to all 3 species. Indicate your reasoning/working in each case. (a) (b) Calculate the rate constant for this reaction at this temperature and give units (c) Discuss the probability of this reaction occurring in a single step. (d) Kinetic studies of reactants are often done under conditions to make them pseudo- first order. Describe what is meant by this term. What reaction conditions would have to be changed to make this study pseudo-first order in l-? The activation energy for this reaction was found to be 84 kJ mol1 at 25 °C. By how must faster would the reaction proceed if the activation energy were lowered bv 10 kJ mol1 (using a suitable catalyst)? (e)
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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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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![Question 5. You are very familiar with the various clock reactions that make iodine in some
form or other. The two you have done in lab use either iodate or iodide as the iodine
"source." However, iodate can be used as a test for iodine according to the reaction:
10: (aq) + 5 1"(aq) + 6 H*(aq) → 3 Iz(aq) + 3 H20(1)
This reaction was studied at 25 °C with different concentrations of the reactants and the
results shown in the Table:
Expt [103] mol dm3
1
[1"] mol dm³
[H*] mol dm³
Rate, mol dm³ s³!
0.10
0.010
0.010
0.60
2
0.10
0.040
0.010
2.40
3
0.30
0.010
0.010
5.40
4
0.10
0.010
0.020
2.40
Use these data to determine the order of the reaction with respect to all 3 species.
Indicate your reasoning/working in each case.
(a)
(b)
Calculate the rate constant for this reaction at this temperature and give units
(c)
Discuss the probability of this reaction occurring in a single step.
(d)
Kinetic studies of reactants are often done under conditions to make them pseudo-
first order. Describe what is meant by this term. What reaction conditions would
have to be changed to make this study pseudo-first order in l-?
The activation energy for this reaction was found to be 84 kJ mol1 at 25 °C. By how
must faster would the reaction proceed if the activation energy were lowered bv 10
kJ mol1 (using a suitable catalyst)?
(e)](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F390bf266-d828-4a8f-b647-4f11f676b241%2F18409d12-c5ae-4fe3-9ea2-7b5b616c2257%2Fkxm0b8e_processed.png&w=3840&q=75)
Transcribed Image Text:Question 5. You are very familiar with the various clock reactions that make iodine in some
form or other. The two you have done in lab use either iodate or iodide as the iodine
"source." However, iodate can be used as a test for iodine according to the reaction:
10: (aq) + 5 1"(aq) + 6 H*(aq) → 3 Iz(aq) + 3 H20(1)
This reaction was studied at 25 °C with different concentrations of the reactants and the
results shown in the Table:
Expt [103] mol dm3
1
[1"] mol dm³
[H*] mol dm³
Rate, mol dm³ s³!
0.10
0.010
0.010
0.60
2
0.10
0.040
0.010
2.40
3
0.30
0.010
0.010
5.40
4
0.10
0.010
0.020
2.40
Use these data to determine the order of the reaction with respect to all 3 species.
Indicate your reasoning/working in each case.
(a)
(b)
Calculate the rate constant for this reaction at this temperature and give units
(c)
Discuss the probability of this reaction occurring in a single step.
(d)
Kinetic studies of reactants are often done under conditions to make them pseudo-
first order. Describe what is meant by this term. What reaction conditions would
have to be changed to make this study pseudo-first order in l-?
The activation energy for this reaction was found to be 84 kJ mol1 at 25 °C. By how
must faster would the reaction proceed if the activation energy were lowered bv 10
kJ mol1 (using a suitable catalyst)?
(e)
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