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A Simple Determination of the NO2 Dimerization Equilibrium Constant

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Qingjiang Yu and Hongxia Gao

Department of Chemistry, Liaocheng Teacher''s College Shandong, China

J. Chem. Educ., 1997, 74 (2), p 233

DOI: 10.1021/ed074p233

Publication Date (Web): February 1, 1997

Section:

History, Education, and Documentation

Abstract

Based on the chemical equilibrium equation

2NO(g) + O₂(g) <--> 2NO₂(g) <--> N₂O₄(g) (1)

this paper deals with the possible gases existing in the reaction system and the change of the total volume of gases after the mixture of two volumes of NO and one volume of O₂ in a closed container under normal pressure (1 atm) with the changes in temperature. Meanwhile, we have obtained an equation for the calculation of the NO₂ polymerization equilibrium constant Kp in the reaction system on the condition that the temperature is within the range of 294.2-413 K and pressure is 1 atm.Kp = [(2V-Vm)Â·Vm]/[4(Vm-V)²]With a glass syringe as the reaction container, we use a water bath to maintain a constant temperature for the determination of the dimerization equilibrium constant of NO. The result of our determination tallies with the documented value.

Keywords (Audience):

Second-Year Undergraduate

Keywords (Domain):

Laboratory Instruction

Keywords (Pedagogy):

Hands-On Learning / Manipulatives

Keywords (Subject):

Equilibrium

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This article has been cited by 1 ACS Journal articles (1 most recent appear below).

Approaching Equilibrium in the N2O4-NO2 System: A Common Mistake in Textbooks
I. A. Leenson
Journal of Chemical Education2000 77 (12), 1652
- Approaching Equilibrium in the N2O4-NO2 System: A Common Mistake in Textbooks
  I. A. Leenson
  Journal of Chemical Education2000 77 (12), 1652
  The paper deals with a widespread mistake in standard textbooks--an experiment with a shift of the equilibrium in gaseous mixtures of nitrogen oxides upon abrupt compression. Any explanation of this experiment should take into account two facts: ...
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