What is the development history of sulfur dioxide? The more detailed, the better.

20 12-08- 19 08:40 History of chemical development-(31) When a volcano erupts, sulfur oxides and hydrogen sulfide will also produce sulfur dioxide, and sulfur dioxide will also become sulfur dioxide when burned in the air. At that time, people didn't know it was sulfur dioxide, only that it was a foul-smelling gas. As early as 1702, chemist Shtal used alkaline solution to absorb the gas produced by sulfur combustion to obtain sulfite solution, so the gas burning sulfur was later called anhydrous sulfurous acid. But because sulfur dioxide can be dissolved in water, it is necessary to wait until the mercury tank is used instead of the water tank to collect this relatively pure gas. 1774, the British chemist priestley made an experiment with sulfuric acid heating. A small amount of mercury and sulfuric acid are heated in a bottle, which produces a large amount of gas before the sulfuric acid boils. Collected in a mercury tank, it smells the same as the last one, can be absorbed by water, and put out candles. Later, he used the heat of copper, iron, silver, sulfur and sulfuric acid respectively to produce this foul-smelling gas. Only then did we know that this gas is composed of sulfur and oxygen.

1772, priestley and Dalton discovered successively that sulfur burns in a closed container filled with mercury, and the volume of gas in the container remains unchanged before and after combustion. This fact is the same as burning charcoal under the same conditions, and the gas volume remains unchanged. It is inferred that anhydrous sulfurous acid is similar to anhydrous carbonic acid, and if it becomes gas, the oxygen contained in their components should be the same. Dalton measured the density of anhydrous sulfurous acid as 2.3 according to the density of oxygen as 1. 1, so he inferred that the weight of sulfur and oxygen in anhydrous sulfurous acid was almost equal. Gay-Lussac heated sulfate at 1807, collected the decomposed gas on a mercury tank, and then treated it with caustic potash. He found that caustic potash absorbed anhydrous sulfurous acid decomposed by sulfate, leaving decomposed oxygen, and found out the ratio of the two in capacity. He uses ferrous sulfate to heat, which is somewhat different from copper sulfate and produces less oxygen. The reason is that the ferrous iron in this compound consumes some oxygen. Gay-Lussac made an experiment with lead sulfate with the same properties. As a result, the volume ratio of anhydrous sulfurous acid decomposed from sulfuric acid to oxygen is about 2 1. If the weight ratio of sulfur to oxygen in anhydrous sulfurous acid is 1: 1, then the weight ratio of sulfur to oxygen (i.e. sulfur trioxide) in anhydrous sulfuric acid is 1: 1.5. This is the weight ratio of sulfur and oxygen in two kinds of sulfur oxides. Because there was no molecular concept at that time, there was only the weight ratio of these two oxide components.