(ii) At elevated temperatures, nitrogen dioxide decomposes to nitric oxide and molecular oxygen:2NO2(g) –→ 2NO(g) + O2(g)The change in concentration of NO2 with time at 300 °C is given below:t (s)100200300400500[NO2]/103(mol dm-3)8.05.64.33.52.92.5By appropriate plotting of the data and use of this graph:(a) verify that this reaction is second order with respect to NO2;(b) determine the rate constant for this reaction.

(a)Order of the reaction can be obtained by plotting the graph. If the plot drawn between…

(ii) At elevated temperatures, nitrogen dioxide decomposes to nitric oxide and molecular oxygen: 2NO2(g) → 2NO(g) + O2(g) The change in concentration of NO2 with time at 300 °C is given below: t (s) 100 200 300 400 500 [NO:J/10-3 (mol dm-3) 8.0 5.6 4.3 3.5 2.9 2.5 By appropriate plotting of the data and use of this graph: (a) verify that this reaction is second order with respect to NO2; (b) determine the rate constant for this reaction.

(ii) At elevated temperatures, nitrogen dioxide decomposes to nitric oxide and molecular oxygen: 2NO2(g) → 2NO(g) + O2(g) The change in concentration of NO2 with time at 300 °C is given below: t (s) 100 200 300 400 500 [NO:J/10-3 (mol dm-3) 8.0 5.6 4.3 3.5 2.9 2.5 By appropriate plotting of the data and use of this graph: (a) verify that this reaction is second order with respect to NO2; (b) determine the rate constant for this reaction.

Chemical Principles in the Laboratory

11th Edition

ISBN:9781305264434

Author:Emil Slowinski, Wayne C. Wolsey, Robert Rossi

Publisher:Emil Slowinski, Wayne C. Wolsey, Robert Rossi

Chapter21: Rates Of Chemical Reactions, Ii. A Clock Reaction

Section: Chapter Questions

Problem 2ASA

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