For the decomposition of nitrous oxide at 565 °C , the rate of the reaction is determined by measuring the appearance of O2.2 N2O 2 N2 + O2At the beginning of the reaction, the concentration of O2 is 0 M. After 18.5 min the concentration has increased to 0.183 M.What is the rate of the reaction? (mol O2 /L) / min For the decomposition of nitrous oxide at 565 °C , the rate of the reaction is determined by measuring the appearance of O22 N20 → 2 N2 +O2At the beginning of the reaction, the concentration of O, is 0 M. After 18.5 min the concentration has increased to 0.183 M.What is the rate of the reaction?| (mol O, /L) / min

2 N2O ---> 2 N2 + O2 For zero order reaction : Rate = [A] – [A0] / Δt Rate = 0.183 M – 0 M /…

Answered: For the decomposition of nitrous oxide…

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 30QAP

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For the decomposition of nitrous oxide at 565 °C , the rate of the reaction is determined by measuring the appearance of O₂.

2 N₂O 2 N₂ + O₂

At the beginning of the reaction, the concentration of O₂ is 0 M. After 18.5 min the concentration has increased to 0.183 M.

What is the rate of the reaction? (mol O₂ /L) / min

For the decomposition of nitrous oxide at 565 °C , the rate of the reaction is determined by measuring the appearance of O2
2 N20 → 2 N2 +O2
At the beginning of the reaction, the concentration of O, is 0 M. After 18.5 min the concentration has increased to 0.183 M.
What is the rate of the reaction?
| (mol O, /L) / min

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