...$k_{298}$^4.1

Units for first order reactions are s$^{-1}$, for the second-order gas reactions are molecules$^{-1}$ cm$^3$ s$^{-1}$, for the third-order gas reactions molecules$^{-2}$ cm$^6$ s$^{-1}$, and for the second-order aqueous reactions are M$^{-1}$ s$^{-1}$. Units for solubility constants are M atm$^{-1}$, and units for dissociation constants are M. Reaction rates are of the form $k = k_{298} \hbox{exp}[-{E \over R} ({1 \over T} - {1 \over 298})]$ unless otherwise noted.

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... &Reference^4.2

NASA97, Demore et al. [49]; Y90, Yin et al. [195,194]; HC85, Hoffmann and Calvert [72]; LK86, Lind and Kok [112]; NBS65, National Bureau of Standards [131]; and M82, Maahs [117].

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... MSA^4.3

Here $k = {{Te^{-234/T} + 8.46\times10^{-10} e^{7230/T} + 2.68\times10^{-10}e^{7810/T}} \over {1.04\times10^{11}T + 88.1e^{7460/T} }}$.

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... ^4.4

Here $k = {{k_{298}\hbox{exp}[-{E \over R} ({1 \over T} - {1 \over 298})] [H^+]} \over {1 + 13[H^+]}}$.

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... time.^6.1

Mid-month concentrations are input and then interpolated to daily values. The input data are constructed to correctly recover the observed monthly means value using the method of Taylor et al. [170]

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