Determining rate law from mechanisms (use the rate-determining step to get the orders). 1. One method for the destruction of ozone in the upper atmosphere is: O3 + NO ® NO2 + O2 (slow) NO2 + O ® NO + O2 (fast) Overall rxn O3 + O ® 2O2 a. Which species is an intermediate? b. Which species is a catalyst? c. Which is the rate-determining step (rds)? d. Number of times each reactant is used in the rds? e. Write the rate law for the reaction.
Determining rate law from mechanisms (use the rate-determining step to get the orders). 1. One method for the destruction of ozone in the upper atmosphere is: O3 + NO ® NO2 + O2 (slow) NO2 + O ® NO + O2 (fast) Overall rxn O3 + O ® 2O2 a. Which species is an intermediate? b. Which species is a catalyst? c. Which is the rate-determining step (rds)? d. Number of times each reactant is used in the rds? e. Write the rate law for the reaction.
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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Determining rate law from mechanisms (use the rate-determining step to get the orders).
1. One method for the destruction of ozone in the upper atmosphere is:
O3 + NO ® NO2 + O2 (slow)
NO2 + O ® NO + O2 (fast)
Overall rxn O3 + O ® 2O2
a. Which species is an intermediate?
b. Which species is a catalyst?
c. Which is the rate-determining step (rds)?
d. Number of times each reactant is used in the rds?
e. Write the rate law for the reaction.
![3) Consider the table of initial rate for the reaction
between hemoglobin (Hb) and carbon monoxide
Experiment [HB]o, mol/L [CO] o, mol/L
1
2.21
1.00
2
4.42
3
3.36
1.00
2.40
h.
Initial Rate, [mol/(L's)
e. Order with respect to HB:
f. Order with respect to CO:
Rate law for this reaction:
0.619
1.24
2.26
Value and units for the rate constant:](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F1ba372ce-f516-407e-85a4-6c51a6a92291%2F0c328a9a-8bff-415b-a546-0726248ee664%2F7h1oifh_processed.jpeg&w=3840&q=75)
Transcribed Image Text:3) Consider the table of initial rate for the reaction
between hemoglobin (Hb) and carbon monoxide
Experiment [HB]o, mol/L [CO] o, mol/L
1
2.21
1.00
2
4.42
3
3.36
1.00
2.40
h.
Initial Rate, [mol/(L's)
e. Order with respect to HB:
f. Order with respect to CO:
Rate law for this reaction:
0.619
1.24
2.26
Value and units for the rate constant:
![Determining rate law from Initial Rates. (Use the ratio of initial
rates to get the orders).
2) Consider the table of initial rates for the reaction: 2C1O₂ +
1-
1-
20H¹ⓇCIO, ¹+ ClO₂ ¹ + H₂O
3
Experiment [C1O2]o, mol/L [OH¹] o, mol/L Initial Rate, mol/(Ls)
1
0.050
0.100
5.75 x 10-²
2
0.100
2.30 x 10¹
3
0.100
1.15 x 10-¹
a.
0.100
0.050
Order with respect to ClO₂:
b. Order with respect to OH¹-:
c. Rate law for this reaction:
d. Value and units for the rate constant:](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F1ba372ce-f516-407e-85a4-6c51a6a92291%2F0c328a9a-8bff-415b-a546-0726248ee664%2Fh8bm1i_processed.jpeg&w=3840&q=75)
Transcribed Image Text:Determining rate law from Initial Rates. (Use the ratio of initial
rates to get the orders).
2) Consider the table of initial rates for the reaction: 2C1O₂ +
1-
1-
20H¹ⓇCIO, ¹+ ClO₂ ¹ + H₂O
3
Experiment [C1O2]o, mol/L [OH¹] o, mol/L Initial Rate, mol/(Ls)
1
0.050
0.100
5.75 x 10-²
2
0.100
2.30 x 10¹
3
0.100
1.15 x 10-¹
a.
0.100
0.050
Order with respect to ClO₂:
b. Order with respect to OH¹-:
c. Rate law for this reaction:
d. Value and units for the rate constant:
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