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Chemical Reactions Producing Hydrogen
"On the Chemical Reaction of Hydrogen Production"
Between heaven and earth, creation is infinite. In the field of chemistry, the reaction of hydrogen production is quite wonderful. Hydrogen is the lightest gas, and it has a wide range of uses.
There is a type of reaction in which metals and acids come into contact, and its effect is very effective. If zinc meets dilute sulfuric acid, it will immediately merge. Zinc is active. Hydrogen ions in sulfuric acid give electricity to zinc, and then form hydrogen atoms. The reaction formula is: $Zn + H_ {2} SO_ {4} = ZnSO_ {4} + H_ {2}\ uparrow $. This reaction is fast and convenient, and is often used in the laboratory to produce hydrogen.
There is also an electrolysis method, which uses water as the source. In water, an electric current is passed, and the water molecules are excited by electricity, which decomposes into hydrogen and oxygen. At the cathode, the hydrogen ions gain electrons and become hydrogen gas; above the anode, the hydroxide ions lose electrons and oxygen escapes. The equation is: $2H_ {2} O\ stackrel {energized }{=\!=\!=} 2H_ {2}\ uparrow + O_ {2}\ uparrow $. Although electricity is required, the hydrogen produced is pure and pure.
In addition, in some chemical reactions, metal hydrides react with water to obtain hydrogen. Sodium hydride reacts rapidly in contact with water. Negative hydrogen ions in sodium hydride combine with hydrogen ions in water, and hydrogen gas is generated. The reaction is as follows: $NaH + H_ {2} O = NaOH + H_ {2}\ uparrow $.
All these chemical reactions for hydrogen production have their own strengths, or are convenient, or pure and good. They are all useful in the chemical industry and energy industry. They contribute greatly to the development of mankind.
Between heaven and earth, creation is infinite. In the field of chemistry, the reaction of hydrogen production is quite wonderful. Hydrogen is the lightest gas, and it has a wide range of uses.
There is a type of reaction in which metals and acids come into contact, and its effect is very effective. If zinc meets dilute sulfuric acid, it will immediately merge. Zinc is active. Hydrogen ions in sulfuric acid give electricity to zinc, and then form hydrogen atoms. The reaction formula is: $Zn + H_ {2} SO_ {4} = ZnSO_ {4} + H_ {2}\ uparrow $. This reaction is fast and convenient, and is often used in the laboratory to produce hydrogen.
There is also an electrolysis method, which uses water as the source. In water, an electric current is passed, and the water molecules are excited by electricity, which decomposes into hydrogen and oxygen. At the cathode, the hydrogen ions gain electrons and become hydrogen gas; above the anode, the hydroxide ions lose electrons and oxygen escapes. The equation is: $2H_ {2} O\ stackrel {energized }{=\!=\!=} 2H_ {2}\ uparrow + O_ {2}\ uparrow $. Although electricity is required, the hydrogen produced is pure and pure.
In addition, in some chemical reactions, metal hydrides react with water to obtain hydrogen. Sodium hydride reacts rapidly in contact with water. Negative hydrogen ions in sodium hydride combine with hydrogen ions in water, and hydrogen gas is generated. The reaction is as follows: $NaH + H_ {2} O = NaOH + H_ {2}\ uparrow $.
All these chemical reactions for hydrogen production have their own strengths, or are convenient, or pure and good. They are all useful in the chemical industry and energy industry. They contribute greatly to the development of mankind.
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