The gas phase decomposition of hydrogen peroxide at 400 °C H2O2(g)---> H2O(g)+ ½O2 (g) is second order in H2O2 with a rate constant of 0.650 1/Mxs . If the initial concentration of H2O2 is 0.176 M, the concentration of H2O2 will be 2.55x10^-2 M after ______ seconds have passed.
The gas phase decomposition of hydrogen peroxide at 400 °C H2O2(g)---> H2O(g)+ ½O2 (g) is second order in H2O2 with a rate constant of 0.650 1/Mxs . If the initial concentration of H2O2 is 0.176 M, the concentration of H2O2 will be 2.55x10^-2 M after ______ seconds have passed.
Chemistry by OpenStax (2015-05-04)
1st Edition
ISBN:9781938168390
Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Chapter12: Kinetics
Section: Chapter Questions
Problem 34E: Use the data provided in a graphical method to determine the order and rate constant of the...
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The gas phase decomposition of hydrogen peroxide at 400 °C
H2O2(g)---> H2O(g)+ ½O2 (g)
is second order in H2O2 with a rate constant of 0.650 1/Mxs .
If the initial concentration of H2O2 is 0.176 M, the concentration of H2O2 will be 2.55x10^-2 M after ______ seconds have passed.
Expert Solution
Step 1
Given,
H2O2(g) ----> H2O(g) + 1/2O2(g)
The reaction is second order.
Rate constant (k) = 0.650 1/M.s
Initial concentration of H2O2 = [H2O2]0 = 0.176 M
Concentration of H2O2 after t sec = [H2O2]t = 2.55 × 10-2 M
Time (t) = ?
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