When combining Ca(OH)2 with Na2CO3 it entraps SO2 out of a gas stream from kiln emissions where ore is processed into nodules. When there is not enough Na2CO3 in this combination, will it not allow the solids to form out and settle?
When combining Ca(OH)2 (calcium hydroxide) with Na2CO3 (sodium carbonate), a chemical reaction takes place, resulting in the formation of solid calcium carbonate (CaCO3) and sodium hydroxide (NaOH). The reaction can be represented by the following equation:
Ca(OH)2 + Na2CO3 -> CaCO3 + 2NaOH
The purpose of this reaction is to remove sulphur dioxide (SO2) from a gas stream in kiln emissions, where ore is being processed into nodules. The reaction traps the SO2 by converting it to calcium sulphite (CaSO3) or calcium sulphate (CaSO4), which can then be removed as a solid.
Now, if there is not enough Na2CO3 in the combination, it means that there is an insufficient amount of sodium carbonate to react with the Ca(OH)2. Consequently, the reaction may not proceed to completion, leading to incomplete conversion of SO2 to solid sulphites or sulphates.
In such a scenario, the solids might not fully form and settle properly. This can result in reduced efficiency in removing SO2 from the gas stream, as the unreacted SO2 and partially formed solids may remain in the gas phase or form smaller particles that are more difficult to collect and separate.
To ensure effective removal of SO2 and proper solid formation, it is crucial to have the appropriate stoichiometric ratio of Ca(OH)2 to Na2CO3 for the desired reaction. Adjusting the quantities of reactants in the right proportion will help optimize the process and increase the efficiency of capturing and removing SO2 from the kiln emissions.