The mechanism for the reaction 2 H2O2(aq) → 2 H2O(1) + O2(g) in thepresence of I (aq) is proposed to bestep 1: H2O2(aq) + I(aq) → H20(1) + Ol (aq) (k1, slow)step 2: H2O2(aq) + Ol (aq) → H20(1) + O2(g) + I"(aq) (k2, fast)Derive the rate law using steady state approximation.O rate =k3[H2O2]?rate = ki [H2O2][1-]rate =ki[H2O]+k2[O2]?rate =k3[O2]

Answered: Image /qna-images/answer/5665e543-c2b2-4985-be71-cc860d776a7a.jpg

Answered: The mechanism for the reaction 2…

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...

See similar textbooks

Similar questions

In aqueous solution buffered at a pH of 6.75 Penicillin G (molecular weight of 334.39 g/mole) undergoes hydrolysis via a pseudo first order reaction that has an activation energy of 77.3 kJ/mole and a pseudo first order rate constant of 1.58 x 10-7 s-1 at 30°C. If a vial of Penicillin G containing 5,000,000 units is stored under the conditions above, how many days will it take for 10% of the drug to hydrolyze?
Hh.191.
Hypothetically, the reaction H2 + 2IC1→ I2+ 2HC1 is first order in [H2] and second order in [ICI]. Based on the first fast step given below and the fact that the second step is the slow step, propose a second-step mechanism, and show that it conforms to the experimentally determined reaction order. Assume that [I2] does not affect the reaction rate. H2 + 2ICI → I2 + 2HC1 Fast: 2ICI → I2 + 2Cl Slow:
The following reaction is first order in respect to CH3OH and first order in respect to HCl. With this in mind, what is the rate constant for the reaction? Be sure you choose the answer with the right units. CH3OH(aq) + HCL(aq) ----> CH3CL(aq) + H2O(i) Reaction CH3OH conc. HCl conc. Initial Rate (M/s) 1 0.100 M 0.100 M 1.1 x 10-2
28. For the aqueous reaction I2 + HPO(OH)2 + H₂O → PO(OH)3 + 2 I¯ + 2 H* the following mechanism is proposed: HPO(OH)₂ P(OH)3 P(OH)3 + 12 → IP(OH)3* + I¯ IP(OH)3 + H₂O → PO(OH)3 + I + 2 H+ fast, unfavorable slow, irreversible fast Which observation is consistent with this mechanism? (A) The reaction is first order in both HPO(OH)2 and I₂. (B) The reaction rate is independent of the I₂ concentration. (C) The reaction goes faster as the concentration of H* is increased. (D) The reaction goes slower as the concentration of I- is increased.
Consider the following proposed reaction mechanism: (1) CIO (aq) + H,O(1)= HCIO(aq) + OH (aq) [fast] (2)I (aq) + HCIO(aq) → HIO(aq) + Cl¯(aq) [slow] (3) OH (aq) + HIO(aq) → H,O() + 10 (aq) [fast] Ignoring water, how many reaction intermediates are present? O 3 O 1 O 2
The overall reaction:S2O82– + 2I – → 2SO42– + I2.can be catalyzed by certain chemical species. Identify the catalyst in the following mechanism:step 1: Fe3+ + 2I – → Fe2+ + I2step 2: S2O82– + Fe2+ → 2SO42– + Fe3+
Pls help ASAP
8. Thallium (1) is oxidized by cerium (IV) as follows: TI+ + 2 Ce+ → T1³+ + 2Ce³+ The elementary steps are as follows: 1. Ce4+ + Mn²+ Ce³+ + Mn³+ 2. Ce4+ + Mn³+ Ce³+ + Mn4+ 3. TI+ + Mn4+ → T1³+ + Mn²+ a) Add all reactants and products and obtain the overall reaction. b) Identify the catalyst and intermediate. c) Determine which is the rate determining step if the rate law for the reaction is Rate = k(Ce4+][ Mn²+]
The rate of consumption of iodide, I-(aq), in the reaction:
In a study of the rearrangement of ammonium cyanate to urea in aqueous solution at 50 °C NH,NCO(aq)→(NH2)½CO(aq) the following data were obtained: [NH,NCO], M |0.715 8.95x10-2 1.05x103 0.358 0.179 minutes 150 449 Hint: It is not necessary to graph these data. (1) The observed half life for this reaction when the starting concentration is 0.715 M is min and when the starting concentration is 0.358 M is min. (2) The average A(1/[NHẠNCO]) / At from t= 0 min to t= 150 min i | The average A(1/[NH,NCO]) / At from t= 150 min to t= 449 min is M min. M' min!. (3) Based on these data, the rate constant for this | order reaction is M' min!.
For a drug to be effective in treating an illnens, its levels in the bloodstream must be maintained for a period of time. One way to measure the level of a drug in the body is to measure its rate of appearance in the urine. The rate of excretion of penicillin is first order, with a half-life of about 30. min. If a person receives an injecction of 21 mg of penicillin at t- 0, how much penicillin remains in the body after 3.0 hours? mg

Recommended textbooks for you

Chemistry

ISBN:

9781305957404

Author:

Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:

Cengage Learning

Chemistry

ISBN:

9781259911156

Author:

Raymond Chang Dr., Jason Overby Professor

Publisher:

McGraw-Hill Education

Principles of Instrumental Analysis

Chemistry

ISBN:

9781305577213

Author:

Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Publisher:

Cengage Learning

Chemistry

ISBN:

9781305957404

Author:

Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:

Cengage Learning

Chemistry

ISBN:

9781259911156

Author:

Raymond Chang Dr., Jason Overby Professor

Publisher:

McGraw-Hill Education

Principles of Instrumental Analysis

Chemistry

ISBN:

9781305577213

Author:

Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Publisher:

Cengage Learning

Organic Chemistry

Chemistry

ISBN:

9780078021558

Author:

Janice Gorzynski Smith Dr.

Publisher:

McGraw-Hill Education

Chemistry: Principles and Reactions

Chemistry

ISBN:

9781305079373

Author:

William L. Masterton, Cecile N. Hurley

Publisher:

Cengage Learning

Elementary Principles of Chemical Processes, Bind…

Chemistry

ISBN:

9781118431221

Author:

Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard

Publisher:

WILEY

SEE MORE TEXTBOOKS