The reaction between ozone and nitrogen dioxide at 231 K is first order in both [NO2] and [O3] 2 NO2(g) + O3(g) → N2O5(g) + O2(g) Express the rate of reaction as a function of the time derivatives of the concentration of all reaction components. Write the rate law for the reaction. If the initial concentration of NO2(g) is tripled, what is the change in the initial reaction rate? What is the effect on reaction rate if the concentration of O3(g) is halved
The reaction between ozone and nitrogen dioxide at 231 K is first order in both [NO2] and [O3] 2 NO2(g) + O3(g) → N2O5(g) + O2(g) Express the rate of reaction as a function of the time derivatives of the concentration of all reaction components. Write the rate law for the reaction. If the initial concentration of NO2(g) is tripled, what is the change in the initial reaction rate? What is the effect on reaction rate if the concentration of O3(g) is halved
Chemistry & Chemical Reactivity
10th Edition
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter14: Chemical Kinetics: The Rates Of Chemical Reactions
Section: Chapter Questions
Problem 17PS: The decomposition of SO2Cl2 is a first-order reaction: SO2Cl2(g) SO2(g) + Cl2(g) The rate constant...
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- The reaction between ozone and nitrogen dioxide at 231 K is first order in both [NO2] and [O3]
2 NO2(g) + O3(g) → N2O5(g) + O2(g)
- Express the
rate of reaction as a function of the time derivatives of the concentration of all reaction components. - Write the rate law for the reaction.
- If the initial concentration of NO2(g) is tripled, what is the change in the initial reaction rate?
What is the effect on reaction rate if the concentration of O3(g) is halved
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