Dissociation Of Hydrogen Sulfide Research Articles

The Free Energy of Sulphur Dioxide

Values of (Fo—E0o)/T for sulphur dioxide are computed from spectroscopic data; the heat of formation of sulphur dioxide from diatomic sulphur and oxygen is calculated from the calorimetric heats of formation of sulphur dioxide and hydrogen sulphide, and Cross' value for the energy of dissociation of hydrogen sulphide. Equilibrium constants for the reactions 12S2(g)+O2=SO2, SO+12O2=SO2are tabulated for the range 298.1 to 2800°K.

Thermodynamic Properties of Sulfur Compounds I. Hydrogen Sulfide, Diatomic Sulfur and the Dissociation of Hydrogen Sulfide

The thermodynamic properties of H2S are calculated from the structure recently obtained by the analysis of an infrared band. — [(F0—E00)/T]*298.1 = 41.174. S*298.1 = 49.151. (Not including the spin contribution.) Montgomery and Kassel's calculations for S2 are corrected in accordance with Badger's new interpretation of the data of Naudé and Christy. — [(F0—E00)/T]298.1 = 47.242. S0298.1 = 54.417. The results are applied to the reaction H2S = H2+½S2. The energy of dissociation of H2S into normal atoms, E00, is found to be 173.8 kg cal. per mole.