The rate law for your reaction is Rate= k[NO2]?. The rate constant for this reaction is 2.5 x 103/M s. If you started out with 0.55M NO2 and you ran the reaction for 5 minutes, what would be the concentration of 4. NO2?
The rate law for your reaction is Rate= k[NO2]?. The rate constant for this reaction is 2.5 x 103/M s. If you started out with 0.55M NO2 and you ran the reaction for 5 minutes, what would be the concentration of 4. NO2?
Chemistry: Principles and Reactions
8th Edition
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:William L. Masterton, Cecile N. Hurley
Chapter11: Rate Of Reaction
Section: Chapter Questions
Problem 28QAP: Diethylhydrazine reacts with iodine according to the following equation: Â...
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Step 1
4)
Given,
Rate law for the reaction,
Rate = k[NO2]2
From rate law we can say that this is a second order reaction.
Initial concentration of NO2 = 0.55 M
Concentration of NO2 after 5 min = ?
Time (t) = 5 min = (5×60) s = 300 s
Rate constant (k) = 2.5 × 10-3/M s
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