https://doi.org/10.1016/j.cej.2012.09.087 In the above reference, process chemistry related to the reactions of CO2 in ammonia solution, the formation of complex ions in the section 2
https://doi.org/10.1016/j.seppur.2022.120786 ” Wang et al. [41] described the reaction between NH3(aq) and CO2(aq), including their equilibria dependent species, and the reversible reactions of ammonium carbamate/ carbamic acid
https://doi.org/10.1039/C9RA00164F ” Fig. 11(a) shows the NH4HCO3(s) mole fraction in the solution at temperatures between 2 and 40 °C and for m(NH3) = 3.1 mol kg−1 H2O. The
https://doi.org/10.1039/C9RA00164F ” Fig. 7 shows the predicted solution speciation and heat of CO2 absorption in the NH3–CO2–H2O system, respectively, all at m(NH3) = 3 mol kg−1 H2O and T = 2
https://doi.org/10.1039/C9RA00164F ” Fig. 6 shows the heat of CO2 absorption predicted by the model and the experimental data of Liu et al.20 and Qin et al.21 at different temperatures. In addition,
https://doi.org/10.1039/C9RA00164F ” Fig. 4 shows the calculated solution speciation and experimental results reported by Lichtfers and Rumpf.60 The corresponding conditions are m(NH3) = 4.44 mol kg−1 H2O and T = 60
https://doi.org/10.1039/C9RA00164F ” Fig. 3 shows the predicted NH3 and CO2 partial pressure at T = 20 °C and different NH3 molality. The model is in good agreement with the experimental data
https://doi.org/10.1039/C9RA00164F ” In order to accurately predict the enthalpy change of each reaction, it is important to obtain accurate chemical equilibrium constants. According to eqn (8),
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