Reaction Rate Review IHydrogen peroxide decomposes to water and oxygen according to the following reaction:H:O: >H:0Its rate of decomposition is measured by titrating samples of the solution with potassiumpermanganate at certain intervals.1. Initial rate determinations at 25 C for the decomposition give the following data[H;O:]0.2000.3000.500Initial rate (mol/L min)1.03 X 1041.55 X 1042.59 X10What is the order of the reaction? Write the rate equation for the decomposition.Calculate the rate constant and the half-life for the reaction at 25 C2. Hydrogen peroxide is sold commercially as a 30.0 % solution. If the solution iskept at room temp. (25 C), how long will it take for the solution to become 10.0% H;O:?3. It has been determined that at 40 C, the rate constant for the reaction is 1.93 X10 /min. Calculate the activation energy for the decomposition of H:O24. Manufacturers recommend that solutions of H:O: be kept in a refrigerator at 4 C.How much longer will it take a 30.0 % solution to decompose to 10.0 % if thesolution is kept in a refrigerator?The rate constant for the catalyzed decomposition of H;O; at 25 C is 2.95 X 10/min. What is the half-life of the catalyzed reaction? What is the rate for thecatalyzed decomposition of 0.500 M H:02?5.6. Hydrogen peroxide in basic solution oxidizes iodide ions to iodine. The proposedmechanism for this reaction isH;O2 - I > HOI+ OH(slow)HOI+ 1+ I + OH(fast)Write the overall redox reaction. Write a rate law consistent with this proposedmechanism.

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Chemistry

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

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

Chapter12: Chemical Kinetics

Section: Chapter Questions

Problem 110CP: Consider a reaction of the type aA products, in which the rate law is found to he rate = k[A]3...

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Reaction Rate Review I
Hydrogen peroxide decomposes to water and oxygen according to the following reaction:
H:O: >
H:0
Its rate of decomposition is measured by titrating samples of the solution with potassium
permanganate at certain intervals.
1. Initial rate determinations at 25 C for the decomposition give the following data
[H;O:]
0.200
0.300
0.500
Initial rate (mol/L min)
1.03 X 104
1.55 X 104
2.59 X
10
What is the order of the reaction? Write the rate equation for the decomposition.
Calculate the rate constant and the half-life for the reaction at 25 C
2. Hydrogen peroxide is sold commercially as a 30.0 % solution. If the solution is
kept at room temp. (25 C), how long will it take for the solution to become 10.0
% H;O:?
3. It has been determined that at 40 C, the rate constant for the reaction is 1.93 X
10 /min. Calculate the activation energy for the decomposition of H:O2
4. Manufacturers recommend that solutions of H:O: be kept in a refrigerator at 4 C.
How much longer will it take a 30.0 % solution to decompose to 10.0 % if the
solution is kept in a refrigerator?
The rate constant for the catalyzed decomposition of H;O; at 25 C is 2.95 X 10
/min. What is the half-life of the catalyzed reaction? What is the rate for the
catalyzed decomposition of 0.500 M H:02?
5.
6. Hydrogen peroxide in basic solution oxidizes iodide ions to iodine. The proposed
mechanism for this reaction is
H;O2 - I > HOI
+ OH
(slow)
HOI
+ 1+ I + OH
(fast)
Write the overall redox reaction. Write a rate law consistent with this proposed
mechanism.

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Hydrogen peroxide decomposes to water and oxygen according to the reaction below:

2 H2O2(aq) → 2 H2O(l) + O2(g)

In the presence of large excesses of I- ion, the following set of data is obtained. What is the average rate of disappearance of H2O2(aq) in M/s in the first 45.0 seconds of the reaction if 1.00 L of H2O2 reacts at 25°C and 1.00 atm pressure?

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