Consider this balanced chemical equation:H2O2(aq) + 3 I - (aq) + 2 H+ (aq)------> I3 - (aq) + 2 H2O(l )In the first 10.0 seconds of the reaction, the concentration of I - drops from 1.000 M to 0.868 M.(a) Calculate the average rate of this reaction in this time interval.(b) Determine the rate of change in the concentration of H+ (that is, Δ[H+]>Δt) during this time interval.
Consider this balanced chemical equation:H2O2(aq) + 3 I - (aq) + 2 H+ (aq)------> I3 - (aq) + 2 H2O(l )In the first 10.0 seconds of the reaction, the concentration of I - drops from 1.000 M to 0.868 M.(a) Calculate the average rate of this reaction in this time interval.(b) Determine the rate of change in the concentration of H+ (that is, Δ[H+]>Δt) during this time interval.
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter11: Chemical Kinetics: Rates Of Reactions
Section: Chapter Questions
Problem 18QRT: Ammonia is produced by the reaction between nitrogen and hydrogen gases. (a) Write a balanced...
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Consider this balanced chemical equation:
H2O2(aq) + 3 I - (aq) + 2 H+ (aq)------> I3 - (aq) + 2 H2O(l )
In the first 10.0 seconds of the reaction, the concentration of I - drops from 1.000 M to 0.868 M.
(a) Calculate the average
(b) Determine the rate of change in the concentration of H+ (that is, Δ[H+]>Δt) during this time interval.
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