Reaction kinetics of carbon dioxide absorption into aqueous potassium salt of histidine

Aqueous amino acid salts are attractive absorbents for carbon dioxide (CO 2 ) capture due to low volatility and resistance to oxidative degradation. The kinetics of CO 2 absorption into aqueous solutions of potassium histidinate (HisK) was investigated using a wetted wall column at concentrations ranging from 0.26 to 2.07   M and temperatures from 298 to 333   K. Density, viscosity of aqueous HisK and physical solubility of N 2 O in these solutions were measured. A temperature dependant ion parameter h His − was correlated to estimate Henry׳s constants of CO 2 . The zwitterion and termolecular mechanisms as well as ionic strength effect on reaction rate were applied to interpret the absorption rate of CO 2 in non-ideal systems. Under the pseudo-first-order regime, the overall reaction rate constants increase strongly with the increasing HisK concentration and temperature. HisK shows comparable chemical reactivity toward CO 2 with the industrial standard monoethanolamine (MEA). The partial reaction order with respect to HisK was found to be an average value of 1.26. Zwitterion deprotonation by water and HisK should be the rate-determining step. Two proposed models from zwitterion and termolecular mechanisms could successfully predict the experimental data within 12% AAD. The activation energy was calculated to be approximately 25.0   kJ   mol −1 .