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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
Chemistry
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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
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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.
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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