Amine Based Solvent for CO Absorption 2 “From Molecular Structure to Process” Prachi Singh Amine Based Solvent for CO 2 Absorption “From Molecular Structure to Process” Prachi Singh Dit proefschrift is goedgekeurd door de promotor: Prof.dr.ir. W. P. M. van Swaaij Samenstelling Promotiecommissie: Voorzitter: Prof.dr. G. van der Steenhoven Universiteit Twente Secretaris: Prof.dr. G. van der Steenhoven Universiteit Twente Promotor: Prof.dr.ir. W. P. M. van Swaaij Universiteit Twente Ass. Promotor: Dr.ir. D. W. F. Brilman Universiteit Twente Referenten: Dr.ir. J. A. Hogendoorn Universiteit Twente Dr.ir. E. Falck da Silva SINTEF, Norway Deskundige: Dr.ir. F. H. Geuzebroek Shell Technology Centre Amsterdam Leden: Prof.dr. S. R. A. Kersten Universiteit Twente Prof.dr.ir. A. Nijmeijer Universiteit Twente Prof.dr.ir. H. J. Heeres Rijksuniversiteit Groningen Dit onderzoek werd financieel ondersteund door nationale projecten CATO Prachi Singh Amine based solvent for CO absorption “From molecular structure to process”. 2 Thesis, University of Twente, The Netherlands ISBN 978-90-365-3200-6 Printed by Wöhrmann Print Service Cover Design: Painting “Green horizon” by Prachi Singh Copyright © 2011 by Prachi Singh All rights reserved. NO part of the material protected by this copyright notice may be reproduced or utilized in any form or by any means, electronic or mechanical, including photocopy, recording or by any information storage and material system, without written permission from the publisher. AMINE BASED SOLVENT FOR CO ABSORPTION 2 “FROM MOLECULAR STRUCTURE TO PROCESS” PROEFSCHRIFT ter verkrijging van de graad van doctor aan de Universiteit Twente, op gezag van de rector magnificus, prof.dr. H. Brinksma, volgens besluit van het College voor Promoties in het openbaar te verdedigen op woensdag 1 juni 2011 om 12.45 uur door Prachi Singh geboren op 29 April 1979 te Meerut, Uttar Pradesh, India Dit proefschrift is goedgekeurd door de promotoren: Prof.dr.ir. W. P. M. van Swaaij Dr.ir. D. W. F. Brilman Dedicated to my Guru Ji Summary Global warming is a well known, worldwide concern, most probably caused by increasing concentrations of CO and other greenhouse gases in the earth’s 2 atmosphere, due to human activities. Especially the production of electricity is a major contributor, responsible for 41% of the world CO emissions in 2008. 2 Worldwide, the power sector relies heavily on coal, the most carbon-intensive of fossil fuels, and hence amplifying its share in global emissions. Carbon Capture and Storage (CCS) offers the opportunity to reduce the CO emissions associated 2 with the use of fossil fuels. Carbon dioxide capture with a regenerable solvent is considered to be a mature technology, since it is successfully applied as CO 2 removal technology in industrial applications. In order to make this technology more economical for post-combustion capture, especially in the power-sector, more research is required to identify solvents which require less energy and lead to lower solvent loss- and corrosion rates in this application. In this thesis, the development of improved, energy efficient amine based solvents is targeted, through experimental (screening) work and by a further understanding of the role of molecular structure on the solvent absorption properties for amine based solvents in a CO absorption process. 2 Primary and secondary amines react with CO forming carbamate-species. The 2 degree of hydrolysis of these carbamate to form bicarbonate depends on several factors, such as its chemical stability, which is influenced by the temperature. Tertiary amines groups cannot react with CO directly to form a carbamate, 2 because these amines lack a free proton. Hence, tertiary amines act as a base and catalyze the hydration of CO , leading to the formation of bicarbonate. Carbamate 2 stability and basicity are the major parameters determining the absorption capacity and regeneration energy requirement. From literature it was identified that steric hindrance is an important parameter in reducing the carbamate stability and is also affecting the basicity of amine based solvents. Steric hindrance is present at different levels (low to high) depending on the number of functional groups substituted at α-carbon next to the amine group. Therefore, the effect of molecular structure like the carbon chain length, functional groups and steric hindrance on the basicity of various amines was studied. It was noticed that for alkanolamine and diamine basicity increases with an increase in carbon chain length, whereas alkyl amine basicity was not affected by an increase in carbon chain length. Difference between two pKa constants for diamines was reduced with an increase in carbon chain length. Steric hindrance showed an increase in the basicity for primary alkanol amines, primary alkylamines and secondary alkylamines, illustrating the clear relationship between the molecular structure and the basicity of the solvents. i The relative carbamate stability for various amine based solvents for CO 2 absorption has been studied by quantum mechanical calculations. Various molecular structure effects like carbon chain length, steric hindrance, functional groups and different configurations of cyclic amines have been investigated using the SM8 solvation model in combination with gas phase reaction energies calculated with the B3LYP density functional method. The trends observed for carbamate stability are (qualitatively) compared with experimental data reported in literature. This work gives theoretical support to the trends observed in earlier experimental studies Singh et al. (2007, 2009) on the effect of the molecular structure. To identify, and to confirm above mentioned-, effects of molecular structure for amine based solvents on their CO absorption capacity and reactivity, solvent 2 screening experiments were performed for CO absorption and regeneration 2 conditions. The absorption of pure CO was performed at 30°C and atmospheric 2 pressure to assess a preliminary indication on the initial absorption rate and absorption capacity (or rich loading). The regeneration of CO from saturated 2 solvents was performed at 80°C and atmospheric pressure to determine the lean loading at pseudo equilibrium. Evaluation of desorption capacity (lean loading) at this relatively low temperature may point out more directly towards a more energy efficient solvent. Results showed that an increase in chain length between the amine and different functional groups in the absorbent structure, results in a decrease of the absorption rate, whereas the absorption capacity was increased in most of the absorbents. A steric hindrance effect was noticed when an alkyl group side chain was present at the alpha–carbon next to the amine group in the absorbent structure. An increase in the number of amine groups, up to 4 amine groups in the absorbent structure, results in an increase of absorption capacity, but also a higher lean loading. Aromatic amines substituted with alkyl groups showed slight increase in an initial absorption rate and absorption capacity. Cyclic saturated diamine substituted with a hydroxyl group by a side chain at the cyclic ring showed the lowest lean loading at pseudo equilibrium when compare to that of other functional group (alkyl or amine) substitution at cyclic ring. Further study was done to evaluate these amine based solvents for CO absorption 2 capacity and reactivity at low CO partial pressure, more close to flue gas 2 emissions conditions. The CO cyclic capacity ( difference in rich and lean CO 2 2 loading) of various potential aqueous amine-based solvents was determined by performing CO absorption experiments at 30°C and 10 kPa CO partial pressure 2 2 and regeneration at 90°C and atmospheric pressure. 1,7-Diaminoheptane and 1,6 Hexanediamine, N,N' dimethyl showed under the conditions studied comparatively high cyclic loadings of 0.81 and 0.85 mole CO /mole amine respectively. Aqueous 2 solutions of 1,6 Hexanediamine, N,N' dimethyl of 0.5 and 2.55 mole/L concentration were selected to study solubility of CO at different CO partial 2 2 pressure ranging from 1 up to 40 kPa, 30°C and at 1 atmosphere. The CO 2 ii