Abstract
In flame gases containing around 1 ppm of total sodium, the concentration of Na atoms is decreased by the addition of a great excess of SO 2 . The decrease is attributed to the formation of a sodium-sulfur-oxygen species, possibly the NaSO 2 radical equilibrated according to the gas-phase reactions NaOH+H=Na+H 2 O NaOH+SO 2 =NaSO 2 +OH On this interpretation, the equilibrium constant for the reaction forming NaSO 2 is K ≅5 exp (-17 kcal/ RT ) at 1500° to 1875°K. A lower temperature and different interaction is observed when flame gases containingaround 100 ppm each of sodium and sulfur are drawn through a quartz probe and the cooled samples are analyzed. The sodium causes a larger decrease of SO 2 than can be explained by the preceding equilibrium. The decrease is independent of the gas temperature before sampling, 1010° to 2100°K, and is therefore considered to occur in the probe and sampling system. It is attributed to a condensation of gaseous NaOH in the cooling gas, and a heterogeneous capture of SO 2 by condensed NaOH. Neither mode of interaction requires the existence of gas-phase Na 2 SO 4 molecules.
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