Hydrogen peroxide decomposes to water and oxygen according to the following reaction: H,O: + H0 + % O 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 104 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
Hydrogen peroxide decomposes to water and oxygen according to the following reaction: H,O: + H0 + % O 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 104 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
Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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Chapter1: Chemical Foundations
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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.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F001a30e7-82ae-4fd9-8c10-f81ad53ce881%2F0f7873b1-31f4-4fe0-8c0e-11bec83944f4%2Faj1z3kl_processed.jpeg&w=3840&q=75)
Transcribed Image Text: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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Follow-up Question
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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