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Equilibrium constant of reaction •OH + HNO3 = H2O + NO3• in aqueous solutionстатья
Информация о цитировании статьи получена из
Web of Science
Дата последнего поиска статьи во внешних источниках: 14 августа 2017 г.
- Авторы: Poskrebyshev G.A., Neta P., Huie R.E.
- Журнал: Journal of Geophysical Research D: Atmospheres
- Том: 106
- Номер: D5
- Год издания: 2001
- Первая страница: 4995
- Последняя страница: 5004
- DOI: 10.1029/2000JD900702
- Аннотация: he equilibrium reaction .OH + HNO3 reversible arrow H2O + NO3. was investigated by pulse radiolysis in aqueous solutions. An estimate of the equilibrium constant was derived from the dependence of the optical absorbance due to NO3. radicals upon the concentration of HNO3. In addition, estimates of the forward and reverse rate constants were obtained from the dependence of the formation rate constant on the ratio of the activities of nitric acid and water. Studies were carried out at different values of the dose per pulse and at pH values of 1 and 0. The observations were modeled, faking into account all relevant reactions for the formation and decay of the nitrate radical. From these modeling studies the estimated rate and equilibrium constants were refined. The rate constant of the forward reaction is found to be (8.6 +/- 1.3) x 10(7) L mol(-1) s(-1), the rate constant of the reverse reaction is found to be (3 +/- 1) X 10(2) L mol(-1) s(-1), and the equilibrium constant K-eq = (2.8 +/- 0.4) x 10(5), all at zero ionic strength. From the latter value of K-eq and taking E-0(H+,(OH)-O-./H2O) = 2.72 V versus NHE, we calculate the reduction potentials E-0(H+, NO3-/HNO3) = (2.40 +/- 0.01) V and E-0(NO3./NO3-) = (2.48 +/- 0.01) V. This value of the reduction potential for this couple leads to a Henry`s law coefficient of K-H = 0.018 mol L-1 bar(-1) at 298 K for NO3.. This value suggests that the impact of NO3. on atmospheric droplets will be due solely to reactive uptake.
- Добавил в систему: Поскрёбышев Григорий Анатольевич