How to obtain sulfuric acid ?
Sulfuric acid - a substance that belongs to a strong dibasic acid.The chemical formula of sulfuric acid - H 2SO4.Pure sulfuric acid - a colorless, oily liquid.Its density is 1.84 g / cm3.The melting temperature is -10.4 degrees Celsius.The chemical properties of this substance promoted that it has become widespread in industry.
Remembering equation sulfuric acid
equations sulfuric acid, describing its receipt, based on the absorption of sulfur oxide (VI) water.Sulfur oxide (VI) SO3- higher sulfur oxide having high reactivity.Reaction of this material with water leads to sulfuric acid.This process is accompanied by a large heat release.
Sulfuric acid can be prepared, for example, of mineral pyrite.This is one of the industrial methods for producing this compound.It is described by the following equations:
- 4FeS2 + 11O2 = 2Fe2O3 + 8SO2
- 2SO2 + O2 = 2SO3
- SO3 + H2O = H2SO4
In this method, as a catalyst in the oxidation of SO2 up of SO3, is used vanadium oxide (V).In addition, the substances are catalysts for the reaction of iron oxide and platinum.However, in the industry they are not used in rationality.Thus, platinum - a very expensive metal.A ferric oxide to exhibit catalytic properties must be heated to a temperature of 625 degrees Celsius.Its use would require additional complexity of the process.Technical
sulfuric acid mixture is, in fact, sulfuric acid and water.The mechanism of oxidation of metals with sulfuric acid depends on its concentration.Thus, if the acid is strongly diluted, it oxidizes hydrogen ion.An example of such a reaction is shown below:
- Zn + H2SO4 = ZnSO4 + H2
This oxidized metals only those whose activity exceeds the activity of hydrogen.If the acid concentration is high, the oxidation takes place at the expense of sulfur.This acid reacts with silver as well as metals that are lower in the electrochemical series of the elements.Thus the final products depend on the activity of the metal and the reaction conditions.Thus, if the metal is inactive, the acid is reduced to sulfur oxide (IV):
- Cu + 2H2SO4 = CuSO4 + SO2 + 2H2O
more active metals may release either sulfur or hydrogen sulfide:
- 3Zn + 4H2SO4 = 3ZnSO4+ S + 4H2O
- 4Zn + 5H2SO4 = 4ZnSO4 + H2S + 4H2O
If you are interested in how to obtain sulfuric acid, the easiest thing to do in a shop.Since the production of it in a home laboratory can not expect to receive a batch, the amount of which is suitable for practical use.