Solubility and diffusivity of N,O and CO, In water were determined as a function of temperature from the results published In the open literature, and new data were measured In the present work. The solubllity of N,O in several aqueous aikanolamlne (DEA, DIPA, DMMEA, and DIPA) solutlons at varlous temperatures was measured and correlated over a wide range of conditions. For both the diffuslvity of N,O and the aikanolamlne In aqueous alkanolamlne solutions a modHled Stokes-Einstein relation was derived. With the ald also of the "N,O analogy" the diffusivity of CO, In these solutlons can be estlmated.

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A study on the reaction between CO2 and alkanolamines in aqueous solutions Blauwhoff, P.M.M.; Versteeg, G.F.; Swaaij, W.P.M. van Abstract-Literature data on the rates of reaction between C0 2 and alkanolamines (MEA, DEA, DIPA, TEA and MDEA) in aqueous solution are discussed . These data induced us to carry out absorption experiments of C02 into aqueous DEA, DIPA, TEA and MDEA solutions from which the respective rate constants were derived . The experimental technique was similar to that used by Laddha and Danckwerts [30] .The results for DEA and DIPA were analysed by means of a zwitterion-mechanism which was derived from the mechanism originally proposed by Danckwerts[16], and were found to fit the model extremely well .The reaction rate of C02 with aqueous TEA and MDEA solutions shows a significant base catalysis effect which is also reported by Donaldson and Nguyen[17] and Barth et at. [ ]. The results for TEA correspond very well with those of Donaldson and Nguyen[171 and Barth et al. [ ] .

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Literature data on the rates of reaction between CO2 and atkanolamines (MEA, DEA, DIPA, TEA and MDEA) in aqueous solution are discussed. These data induced us to carry out absorption experiments of CO-r into aqueous DEA, DIPA, TEA and MDEA solutions from which the respective rate constants were derived. The experimental technique was similar to that used by Laddha and Daockwerts[30]. The results for DEA and DIPA were analysed by means of a zwitterion-mechanism which was derived from the mechanism originally proposed by Danckwerts[l6], and were found to fit the model extremely well. The reaction rate of CO* with aqueous TEA and MDEA solutions shows a significant base catalysis effect which is.also reported by Donaldson and Nguyen[l7] and Barth et al. [4]. The results For TEA correspond very well with those of Donaldson and Nguyen[lfl and Barth et al.[4]. REVIEW OF LITERATURE KINETIC DATA General remarks Comparison of literature data on kinetics of CO?alkanolamine reactions is a complicated matter, because the authors use different experimental techniques. physico-chemical data and amine purities. The latter factor is usually overlooked, but even very small amounts of primary amine contaminants in secondary amines and ces VOI 39. No. 2-A 207

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The reaction of CO, with TEA, DMMEA, and DEMEA has been studied at 293, 303, 318 and 333 K. All the kinetic experiments were carried out in a stirred cell reactor operated with a flat, smooth and horizontal gas-liquid interface. A numerical method, which describes mass transfer accompanied by reversible chemical reactions, has been applied to infer rate constants from the experimental data. It is argued that the contribution of the CO, reaction with OH-to the observed reaction rate may have been overestimated in most literature on tertiary amine kinetics as serious depletion of OH-toward the gas-liquid interface usually occurs.For all the amines studied, the reaction order in amine was found to be about one for each temperature investigated. This is in good agreement with the base catalysis mechanism proposed by Donaldson and Nguyen (1980). All kinetic data could be summarized reasonably well in one BrBnsted relationship. R. J. Littel