---------- (see attached image) ----------Questions:How long does it take for one-half of a 0.882 M hydrogen peroxide solution to decompose? (The decomposition of hydrogen peroxide is a first order reaction with k= 0.0410 min-1).How long does it take for one-half of a 0.441 M hydrogen peroxide solution to decompose? III: Half-lifeThe half-life of a chemical is the time required to reduce the concentration by 50%. Theequations are as follows:Half-Life EquationsZero order (rate k):%3D1[A].0802 kFirst order (rate = k [A]):%3D0.693kSecond order (rate = k [A]²):1K[A).

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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...

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Questions:

How long does it take for one-half of a 0.882 M hydrogen peroxide solution to decompose? (The decomposition of hydrogen peroxide is a first order reaction with k= 0.0410 min-1).
How long does it take for one-half of a 0.441 M hydrogen peroxide solution to decompose?

III: Half-life
The half-life of a chemical is the time required to reduce the concentration by 50%. The
equations are as follows:
Half-Life Equations
Zero order (rate k):
%3D
1[A].
080
2 k
First order (rate = k [A]):
%3D
0.693
k
Second order (rate = k [A]²):
1
K[A).

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