The decomposition of hydrogen peroxide is a first-order reaction: H2O2(aq) H2O(l) + 1 / 2 O2(g)

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The decomposition of hydrogen peroxide is a first-order reaction:

H2O2(aq) → H2O(l) + 1 / 2 O2(g)

The half-life of the reaction is 17.0 minutes.

a. What is the rate constant of the reaction?

b. If you had a bottle of H2O2, how long would it take for 86.0% to decompose?

c. If you started the reaction with [H2O2] = 0.100 M, what would be the hydrogen peroxide concentration after 15.0 minutes?

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General Chemistry

ISBN: 978-1439043998

9th edition

Authors: Darrell Ebbing, Steven D. Gammon

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Question Posted: Mar 01, 2016 04:31 AM

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The decomposition of hydrogen peroxide is a first-order reaction: H2O2(aq) H2O(l) + 1 / 2 O2(g)

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a k ln2 t 12 0693 170 min 004076 00408 min b When 860 of the ...View the full answer

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