CaO+SO2+H2O-->CaSO3+H2O
SO2 (g) + CaO (s) ----> CaSO3
S +o2 => so2
Yes of course Ca(OH)2 could replace NaOH to have the following reactions Ca(OH)2 + SO2 = CaSO3 + H2O CaSO3 +1/2 O2 + 2H2O = CaSO4.2H2O
4FeS + 7O2 = 2Fe2O3 + 4SO2
CaO+SO2+H2O-->CaSO3+H2O
This equation is 2 CaCO3 + 2 SO2 + O2 -> 2 CaSO4 + 2 CO2.
SO2 (g) + CaO (s) ----> CaSO3
Sulfur dioxide can be removed from a gas phase by making use of the reaction SO2 + CaO = CaSO3.
Under very specific circumstances it can, however, the normal reaction between CaSO3 and heat in the presence of O2 (in air, for example) is to create CaSO4. A good example is the dry lime flue gas desulfurization process. In a non-forced oxidation process, CaO (lime) readily reacts with SO2 forming CaSO3 in flue gas, which is then recovered as a solid. With added oxygen (the forced oxidation process), the CaSO3 in the flue gas oxidizes to CaSO4, which is then recovered as a solid. In air, even at room temperatures, CaSO3 slowly oxidizes to CaSO4. That said, in order to get from CaSO3 to CaO and SO2, you have to heat it under reducing conditions to drive off the oxygen, creating CaS, cleave the Ca-S bond, then perform an oxidation reaction to form recoverable CaO and SO2.
S +o2 => so2
Yes of course Ca(OH)2 could replace NaOH to have the following reactions Ca(OH)2 + SO2 = CaSO3 + H2O CaSO3 +1/2 O2 + 2H2O = CaSO4.2H2O
yeah
4FeS + 7O2 = 2Fe2O3 + 4SO2
Under most circumstances sulphur burns to give SO2. Limestone will not burn but can decompose to leave CaO. Heated together in the presence of air, another product might be CaSO3. Without defining what constitutes a product, defining a by-product is impossible.
It combines with it in the following reaction: SO2 + Ca(OH)2 --> CaSO3 + H2O
there are more oxygen atoms on one side than on the other