The decomposition rate of sodium
hydrogen carbonate (NaHCO3) into carbonate (Na2CO3) was determined as weight loss at ambient pressure
and elevated temperatures up to 230 °C. A particularly slow increasing-temperature
procedure and small samples of fine powders were employed to minimize
heat and mass transfer intrusions. Efficient removal of the gaseous
products eliminated possible equilibrium constraints. A near-first-order
reaction rate equation has been presented for the decomposition reaction
and also verified by the data collected by experiment in a constant-temperature
mode. This correlation makes it possible to predict the reaction rate
as a function of temperature and the extent of decomposition. In combination
with its integrated form, it can readily be used, for example, in
modeling or design of the decomposition process. Experimental measurements
show that the porosity of parent (precursor) solids persists during
the calcination process. It is believed that such a highly alkaline
porous reactant is sort of ideally suited for the fast sorption of
unwanted acid gases. The sintering of the nascent NaHCO3-derived carbonate was explored in a nitrogen environment at temperatures
from 120 to 230 °C. An empirical model has been proposed to correlate
the experimental results on the most probable pore diameter, the specific
surface area, and the micrograin size of calcines in dependence upon
the temperature of sintering. In addition to the pore volume, also
these textural/structural features are of considerable importance
in assessment of the sorbent suitability.
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