| OCR Text |
Show 1990 AFRC Int'l Symposium described by van't Hoff's law of mobile equilibrium). Figure 12 offers a graphical description of the temperature dependence of C12 and NO solubilities in water. As may be seen, the solubility of C12 is a couple of orders of magnitude larger than that of NO. This disparity increases as the ionic strength of the solvent increases. The solubility of NO will decrease somewhat more if the electrolytic solution has a relatively low (S2) pH level. Interestingly, in HCl solutions, the solubility curve of C12 has an unusual feature, which is highlighted in Figure 13. The solubility of C12 is depressed in a region from approx. 0.1 to 1M. Then, rather than continuing to negatively influence the solubility of C12 (as one would predict from the results of apparent hydrolysis thermodynamic reactions), the solubility increases linearly with increases in HCl solvent concentration. This increase in chlorine solubility is due to the complexing of diatomic chlorine with solubilized chloride ion (Cl-) to form trichloride ion, as will be discussed in the next section. It is concluded that NO is a relatively insoluble gas species in a large variety of electrolytic aqueous-based solvents. Thus, enhanced solubility and, subsequently, increased absorption/removal of NO from the gas stream due to increased ionic strength of the scrubber fluids is not the reason C12 injection followed by aqueous scrubbing is such an effective NO removal technique, as was made evident by the experimental data. The answer lies in the reaction and interaction 0 N x ~ 0 0 ,M ~ ~ ~ ~ 0 ~ ~ ~ ~ ~ ~ ~ ~ ~ 0 ~ ~ ~ ~ Solubility of chlorine and nitric oxide as a function of temperature 1.5000 \ \ 1.0000 \\ ~ C1 2 0.5000 --- --- ---- --- 0.0000 " 0.0 20.0 40. 0 60.0 80.0 T, °c Figure 12 " of NO with the hydrolysis products of C12 at the gas-liquid interface. -10- 100.0 |
