The chemical equation for the production of hydrogen in the laboratory

zn+h2so4=znso4+h2↑

Use a test tube, put zinc particles (Zn), then slowly pour sulfuric acid (H2SO4), plug a rubber plug at the mouth of the test tube, and pass the catheter into the gas collection cylinder to collect hydrogen. (It is better not to use hydrochloric acid, as this will collect some HCl gas).

Experimental principle: The hydrogen gas produced by the reaction of active metals and dilute sulfuric acid is usually made with metal zinc and dilute sulfuric acid or dilute hydrochloric acid.

Precautions: 1) When potassium, calcium, sodium and other metals react with dilute acid, they will preferentially replace the hydrogen in the water and form the corresponding alkali, and the reaction is too violent.

2) The selected metal should react with the acid at a moderate rate and produce uniform bubbles.

3) Nitric acid or concentrated sulfuric acid should not be used, because these two acids have strong oxidizing properties, and the reaction will produce NO2 or SO2.

Hydrogen equation for laboratory production:

1. Reaction with zinc and dilute sulfuric acid to generate hydrogen, chemical reaction formula: Zn + H2SO4 = ZnSO4 + H2, the principle of this method is mainly to use zinc to be more active than hydrogen, and the reaction with sulfuric acid will replace hydrogen to generate hydrogen, which is currently the most commonly used method for making hydrogen in the laboratory.

2. Hydrogen is generated by reaction of zinc and hydrochloric acid, and the chemical reaction formula is: 2zn+2HCl=2znCl2+H2

3. Hydrogen is prepared by reaction of aluminum and sodium hydroxide solution, and the chemical reaction formula is: 2Al + 2NaOH + 2H2O = 2Naalo2 (sodium metaaluminate) + 3H2.

4. Hydrogen is produced by electrolysis of water, chemical reaction formula: 2H2O=O2 +2H2, the principle of this method is mainly to use ionization energy to ionize hydrogen and hydrogen, the cost of this method is high, and it is not commonly used in the laboratory.

Areas of application of hydrogen:

Because hydrogen has good reducing property and no pollution, hydrogen can be used as a reducing agent instead of carbon in metal smelting; In addition, hydrogen can also be used in the production of optical fibers, metal cutting and welding, hydrogen fuel cell vehicles, distributed power generation, etc.

In general, hydrogen is readily bound to oxygen. This property makes it a natural reducing agent for use in production to prevent oxidation. In high-temperature processing of glass manufacturing and in the manufacture of electronic microchips, hydrogen is added to nitrogen shielding gas to remove residual oxygen.

In the petrochemical industry, hydrogenation is required for refining by desulfurization and hydrocracking**. Another important use of hydrogen is the hydrogenation of fats in margarine, cooking oils, shampoos, lubricants, household cleaners, and other products.

The above content reference: Encyclopedia - Hydrogen.

The equation for laboratory chemistry is: Zn+H2SO4=ZnSO4+H2.

There are two ways to produce hydrogen in chemical laboratories, one is by electrolysis of water.

to produce hydrogen (H2) and also produce oxygen.

The chemical equation is: 2H2O (energized)2H2 DecaO2. The other is to use specific hydrogen elements.

It is a reactive metal element, which undergoes a displacement reaction with acid.

The equation for this type of reaction is: Zn deca 2HCl Znc 2 dec H2 , Fe deca H2SO4 FeSO4 dec H2 .

1. Reaction between metals and acids.

zn+h2so4=znso4+h2↑

2. Reaction between metal and alkali.

2al+2naoh+2h2o=2naalo2+3h2 3, electrolysis. 2NaCl + 2H2O == (energized) = 2NaOH + Cl2 + H2

Zinc and dilute sulfuric acid are often used to produce hydrogen in the laboratory, and zinc and dilute sulfuric acid react at room temperature to produce zinc sulfate and hydrogen, and the chemical equation of the reaction is: Zn + H2SO4 Zn SO4 + H2.

Hydrogen is stable at room temperature, and can react with many substances under the condition of ignition or heating.

Flammability (can be burned in oxygen or chlorine): 2H2 + O2 = ignition = 2H2O (chemical reaction).

Ignition of impure hydrogen gas can occur**, it must be verified before hydrogen is ignited, similarly, deuterium (heavy hydrogen) ignited in oxygen can produce heavy water (D2O)).

H2 + Cl2 = ignition = 2HCl (chemical reaction) In this reaction, the combustion flame is pale and white under light conditions**.

H2+F2=2HF (Hydrogen and fluorine are mixed to form hydrogen fluoride gas immediately, even under dark conditions).

Reducibility (e.g. reducing certain metal oxides).

H2 + Cuo Cu + H2O (displacement reaction).

3H2 + Fe2O3 = High temperature = 2Fe + 3H2O (displacement reaction).

3H2 + WO3 W + 3H2O (displacement reaction).

Hydrogen can also undergo addition reactions with double or triple bonds.