Thermodynamics

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),

https://doi.org/10.1039/C9RA00164F ” The heat of each individual reaction ((R1)–(R7)) is expressed in terms of enthalpy change, ΔHk, which can be calculated from the van’t Hoff’s

https://doi.org/10.1039/C9RA00164F ” It is difficult to experimentally determine each individual reaction’s contribution to the overall heat of CO2 absorption. Thermodynamic analysis is proved to be a