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Hydrogen properties and use of hydrogen

Hydrogen properties and use of hydrogen

There are numerous other uses for hydrogen. It is used to make cyclohexane and methanol, which are intermediates in the production of plastics and pharmaceuticals, and ammonia for agricultural fertilizer (the Haber process). During the oil-refining process, it is also used to remove sulfur from fuels.

Due to its similarity to alkali metals and halogens, hydrogen is a unique element in the periodic table.

Because it is unique, hydrogen is placed separately on the periodic table as the first element. Allow us to see a few reasons in view of which Hydrogen is so remarkable.

Properties of Hydrogen

Due to its dual nature, hydrogen is widely used in the chemical industry because of its numerous applications. In this way, let us view its properties and track down the explanations behind its double person:

Physical properties of Hydrogen:

The hydrogen gas is colorless, has no smell, and has no taste. It is a gas that can be burned, but it does not support combustion. It is insoluble in water and lighter than air. It has a nuclear mass of 1.008 amu and an ionization enthalpy of 1312 kJ mol-1.

Chemical properties of Hydrogen:

The bond dissociation enthalpy is largely responsible for determining chemical properties. The bond enthalpy between two atoms of an element is highest when hydrogen molecules form an H-H bond. Because hydrogen has a high bond enthalpy and is inert at room temperature, it must be prepared at extremely high temperatures in an electric arc or under ultraviolet light. Because hydrogen has an electronic configuration of 1s1, it can react by either losing an electron and forming an H+ ion or by gaining an electron and forming an H– ion. Both of these reactions are possible. Covalent bonds are formed when hydrogen and other elements share electrons.

Reaction of Hydrogen with Other Elements

Let us move on to the reaction of hydrogen with other elements:

Reactions with the halogen family:

Hydrogen reacts with halogens elements to give hydrogen halides.
For example:

Reaction with the oxygen molecule:

Hydrogen reacts with the oxygen molecule to form water. This reaction is highly exothermic in nature.

Reaction with metals:

Hydrogen reacts with different metals to form their respective hydrides.

here M represents the alkali metals.

Uses of Hydrogen

Hydrogen finds a variety of application due to its dual nature. Following are some important uses of hydrogen:

Hydrogen is utilized in the combination of alkali and the production of nitrogenous composts.
Production of vanaspati fat through the hydrogenation of unsaturated vegetable oils.
It is utilized in the production of numerous organic compounds, including methanol.
Hydrogen is used to make hydrogen chloride, a very useful chemical.
Through metallurgical processes, hydrogen can transform numerous metal oxides into metals.
Numerous activities related to space research make use of hydrogen as rocket fuel.
The automotive industry is testing hydrogen fuel using hydrogen fuel cells.

Why do we need hydrogen?

Hydrogen is a significant water element. The body’s cells remain hydrated due to water and help remove toxins from the body. Hydrogen enables the body to produce energy.

Who discovered hydrogen?

Robert Boyle produced hydrogen gas in 1671 while experimenting with acids and iron, but Henry Cavendish didn’t acknowledge it as a separate component until 1766, according to Jefferson Lab. Antoine Lavoisier, a French chemist, gave the element hydrogen the name

How does hydrogen exist in nature?

On Earth, hydrogen is mostly found in the form of water. Two hydrogen atoms and one oxygen atom make up each H2O water molecule.

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