Overall Reaction: FeCl2 + Oz' + HCl → Cl¿FEO2H + Cl CI. CI-Fe-CI 0=0 HCI `Fe-O-OH rate = (1.096 M's') [FeCl2][O2] Mechanism 1: 0; + HCI $ HỌ, + CH FeCl, + HO, → CI,Fe-O,H (fast) (slow) (very fast) CI,Fe-O,H + CI → ClFe-O,H + CI, In the trials below, the temperature of the reaction was varied and concentrations held constant at: [FeCl,] is 0.025 M, (02`) is 0.17 M, and (HCl] is 0.022 M. Mechanism 2: Initial Rate of Reaction Temperature FeCl, + 0; Cl,Fe-O, CI,Fe-O, + HCI → CI,Fe-O,H + CI- (fast) (slow) 4.66 x 10° M/s 7.68 x 10* M/s 2.37 x 10 M/s 25ºC 7 °C 42 °C Mechanism 3: FeCl, + 0; → C,Fe-O, CI,Fe-O, + HCI → CI,Fe-O,H + Cl (slow) (fast) 1. Predict the rate law for each possible mechanism. 2. Compare the predicted rate laws with the experimentally determined rate law. 3. Calculate the activation energy for the rate determining step. 4. Assume the enthalpy of the reaction is -50.0 kJ/mole. Draw the reaction diagram.
Overall Reaction: FeCl2 + Oz' + HCl → Cl¿FEO2H + Cl CI. CI-Fe-CI 0=0 HCI `Fe-O-OH rate = (1.096 M's') [FeCl2][O2] Mechanism 1: 0; + HCI $ HỌ, + CH FeCl, + HO, → CI,Fe-O,H (fast) (slow) (very fast) CI,Fe-O,H + CI → ClFe-O,H + CI, In the trials below, the temperature of the reaction was varied and concentrations held constant at: [FeCl,] is 0.025 M, (02`) is 0.17 M, and (HCl] is 0.022 M. Mechanism 2: Initial Rate of Reaction Temperature FeCl, + 0; Cl,Fe-O, CI,Fe-O, + HCI → CI,Fe-O,H + CI- (fast) (slow) 4.66 x 10° M/s 7.68 x 10* M/s 2.37 x 10 M/s 25ºC 7 °C 42 °C Mechanism 3: FeCl, + 0; → C,Fe-O, CI,Fe-O, + HCI → CI,Fe-O,H + Cl (slow) (fast) 1. Predict the rate law for each possible mechanism. 2. Compare the predicted rate laws with the experimentally determined rate law. 3. Calculate the activation energy for the rate determining step. 4. Assume the enthalpy of the reaction is -50.0 kJ/mole. Draw the reaction diagram.
Chemistry
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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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Please help me with question 3 and 4. Thank you.
![Overall Reaction: FeCl2 + Oz° + HCl → Cl½FeO2H + Cl
CI
Fe-O-OH
CI-Fe-CI
HCI
rate = (1.096 M1s1) [FeClz][O2]
%3D
Mechanism 1:
0; + HCI S HO, + CI
FeCl, + HO, → CI,Fe-O,H
CI,Fe-O,H + CI → ClFe-O,H + Cl,
(fast)
(slow)
(very fast)
In the trials below, the temperature of the reaction
was varied and concentrations held constant at:
[FeCl,] is 0.025 M, [O2 ] is 0.17 M, and [HCl] is 0.022 M.
Mechanism 2:
Initial Rate of Reaction
Temperature
FeCl, + 0; 5 CI,Fe-O,
CI,Fe-O, + HCI → Cl,Fe-O,H + Cl-
(fast)
(slow)
4.66 x 10° M/s
7.68 x 10* M/s
2.37 x 102 M/s
25°C
7 °C
42 °C
Mechanism 3:
FeCl, + 0; → CI,Fe-O,
CI,Fe-O, + HCI→ CI,Fe-O,H + CH
(slow)
(fast)
1. Predict the rate law for each possible mechanism.
2. Compare the predicted rate laws with the experimentally determined rate law.
3. Calculate the activation energy for the rate determining step.
4. Assume the enthalpy of the reaction is -50.0 kJ/mole. Draw the reaction diagram.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fa49e8544-22cd-49e6-b20c-ed062c173676%2Fa47d35aa-fb70-4a45-acda-69fe13ed8353%2F1u1n8pf_processed.png&w=3840&q=75)
Transcribed Image Text:Overall Reaction: FeCl2 + Oz° + HCl → Cl½FeO2H + Cl
CI
Fe-O-OH
CI-Fe-CI
HCI
rate = (1.096 M1s1) [FeClz][O2]
%3D
Mechanism 1:
0; + HCI S HO, + CI
FeCl, + HO, → CI,Fe-O,H
CI,Fe-O,H + CI → ClFe-O,H + Cl,
(fast)
(slow)
(very fast)
In the trials below, the temperature of the reaction
was varied and concentrations held constant at:
[FeCl,] is 0.025 M, [O2 ] is 0.17 M, and [HCl] is 0.022 M.
Mechanism 2:
Initial Rate of Reaction
Temperature
FeCl, + 0; 5 CI,Fe-O,
CI,Fe-O, + HCI → Cl,Fe-O,H + Cl-
(fast)
(slow)
4.66 x 10° M/s
7.68 x 10* M/s
2.37 x 102 M/s
25°C
7 °C
42 °C
Mechanism 3:
FeCl, + 0; → CI,Fe-O,
CI,Fe-O, + HCI→ CI,Fe-O,H + CH
(slow)
(fast)
1. Predict the rate law for each possible mechanism.
2. Compare the predicted rate laws with the experimentally determined rate law.
3. Calculate the activation energy for the rate determining step.
4. Assume the enthalpy of the reaction is -50.0 kJ/mole. Draw the reaction diagram.
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Arrhenius equation explains the variation in rate of the reaction with change in temperature.
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