Dinitrogen pentoxide (N2O5) decomposes in chloroformas a solvent to yield NO2 and O2. The decomposition isfirst order with a rate constant at 45 °C of 1.0 x 10-5 s-1.Calculate the partial pressure of O2 produced from 1.00 Lof 0.600 M N2O5 solution at 45 °C over a period of 20.0 hif the gas is collected in a 10.0-L container. (Assume thatthe products do not dissolve in chloroform.)
Dinitrogen pentoxide (N2O5) decomposes in chloroformas a solvent to yield NO2 and O2. The decomposition isfirst order with a rate constant at 45 °C of 1.0 x 10-5 s-1.Calculate the partial pressure of O2 produced from 1.00 Lof 0.600 M N2O5 solution at 45 °C over a period of 20.0 hif the gas is collected in a 10.0-L container. (Assume thatthe products do not dissolve in chloroform.)
Principles of Modern Chemistry
8th Edition
ISBN:9781305079113
Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Chapter18: Chemical Kinetics
Section: Chapter Questions
Problem 9P
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Dinitrogen pentoxide (N2O5) decomposes in chloroform
as a solvent to yield NO2 and O2. The decomposition is
first order with a rate constant at 45 °C of 1.0 x 10-5 s-1.
Calculate the partial pressure of O2 produced from 1.00 L
of 0.600 M N2O5 solution at 45 °C over a period of 20.0 h
if the gas is collected in a 10.0-L container. (Assume that
the products do not dissolve in chloroform.)
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