Kinetics of the sodium carbonate–sulfur dioxide reaction

AIChE Journal ◽  
1987 ◽  
Vol 33 (9) ◽  
pp. 1522-1532 ◽  
Author(s):  
Shoichi Kimura ◽  
J. M. Smith
Keyword(s):  
Sulfur Dioxide ◽  
Sodium Carbonate ◽  
Kinetics Of

The Reactivity of Different Active Forms of Sodium Carbonate with Respect to Sulfur Dioxide

1992 ◽  
Vol 57 (11) ◽  
pp. 2302-2308
Author(s):  
Karel Mocek ◽  
Erich Lippert ◽  
Emerich Erdös
Keyword(s):  
Thermal Decomposition ◽  
Liquid Phase ◽  
Sulfur Dioxide ◽  
Specific Surface ◽  
Surface Area ◽  
Sodium Carbonate ◽  
Room Temperature ◽  
Active Form ◽  
The Other ◽  
Kinetics Of

The kinetics of the reaction of solid sodium carbonate with sulfur dioxide depends on the microstructure of the solid, which in turn is affected by the way and conditions of its preparation. The active form, analogous to that obtained by thermal decomposition of NaHCO3, emerges from the dehydration of Na2CO3 . 10 H2O in a vacuum or its weathering in air at room temperature. The two active forms are porous and have approximately the same specific surface area. Partial hydration of the active Na2CO3 in air at room temperature followed by thermal dehydration does not bring about a significant decrease in reactivity. On the other hand, if the preparation of anhydrous Na2CO3 involves, partly or completely, the liquid phase, the reactivity of the product is substantially lower.

The effect of particle size on the reactivity of active sodium carbonate towards sulfur dioxide

1979 ◽  
Vol 44 (12) ◽  
pp. 3419-3424
Author(s):  
Karel Mocek ◽  
Erich Lippert ◽  
Dušan Husek ◽  
Emerich Erdös
Keyword(s):  
Particle Size ◽  
Sulfur Dioxide ◽  
Sodium Carbonate ◽  
Reaction Rate ◽  
Active Form ◽  
Controlling Factor ◽  
Active Sodium ◽  
Effect Of Particle Size ◽  
Integral Reactor

The effect of particle size (0.33-1.0 mm) of the sodium carbonate on the reactivity of the active sodium carbonate prepared therefrom towards the sulfur dioxide was studied in a fixedbed integral reactor at a temperature of 150 °C. The found dependence of the reaction rate on the particle size exhibits an unexpected course; at sizes of about 0.65 mm, a distinct minimum appears. The reaction rate decreases approximately ten times in the first branch of this dependence. The controlling factor of the reactivity of sodium carbonate, however, remains to be the method of preparing the active form.

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