Preparation of hydrogen

Preparation of hydrogen

Hydrogen

Hydrogen is the most abundant element in the universe. The sun and other stars are composed largely of hydrogen. Astronomers estimate that 90% of the atoms in the universe are hydrogen atoms. Hydrogen is a component of more compounds than any other element. Water is the most abundant compound of hydrogen found on earth. Hydrogen is an important part of petroleum, many minerals, cellulose and starch, sugar, fats, oils, alcohols, acids, and thousands of other substances.

At ordinary temperatures, hydrogen is a colorless, odorless, tasteless, and nonpoisonous gas consisting of the diatomic molecule H₂. Hydrogen is composed of three isotopes, and unlike other elements, these isotopes have different names and chemical symbols: protium, ¹H, deuterium, ²H (or “D”), and tritium ³H (or “T”). In a naturally occurring sample of hydrogen, there is one atom of deuterium for every 7000 H atoms and one atom of radioactive tritium for every 10¹⁸ H atoms. The chemical properties of the different isotopes are very similar because they have identical electron structures, but they differ in some physical properties because of their differing atomic masses. Elemental deuterium and tritium have lower vapor pressure than ordinary hydrogen. Consequently, when liquid hydrogen evaporates, the heavier isotopes are concentrated in the last portions to evaporate. Electrolysis of heavy water, D₂O, yields deuterium. Most tritium originates from nuclear reactions.

 

Preparation of Hydrogen

Elemental hydrogen must be prepared from compounds by breaking chemical bonds. The most common methods of preparing hydrogen follow.

From Steam and Carbon or Hydrocarbons

Water is the cheapest and most abundant source of hydrogen. Passing steam over coke (an impure form of elemental carbon) at 1000 °C produces a mixture of carbon monoxide and hydrogen known as water gas:

 

Water gas is as an industrial fuel. It is possible to produce additional hydrogen by mixing the water gas with steam in the presence of a catalyst to convert the CO to CO₂. This reaction is the water gas shift reaction.

It is also possible to prepare a mixture of hydrogen and carbon monoxide by passing hydrocarbons from natural gas or petroleum and steam over a nickel-based catalyst. Propane is an example of a hydrocarbon reactant:

 

Electrolysis

Hydrogen forms when direct current electricity passes through water containing an electrolyte such as H₂SO₄, as illustrated . Bubbles of hydrogen form at the cathode, and oxygen evolves at the anode. The net reaction is:

Physical properties of hydrogen:

– Hydrogen is a colorless, odourless and tasteless gas which is sparingly soluble in water.
– Hydrogen is the lightest gas.
– Density: 0.8987 gram per litre
– Boiling point: -253^oC
– Melting point: -259^oC
– It can be liquefied and solidified at low temperature and high pressure

 

Chemical properties:

1. Action with indicators: It does not show any reaction with litmus and hence is neutral towards litmus paper andother indicators.
2. Combustibility:Hydrogen is a inflammable and combustible gas. It is non supporter of combustion.
   It gives pale blue flame in air or oxygen to form water. So, hydrogen is also called water gas.

2H2+O2⟶H2O2H2+O2⟶H2O

3. Dissociation:Hydrogen is quiet stable to its high bond energy. It dissociates into atomic hydrogen atoms when heated above1730 ^o.

ZnSO4−→−−−−>1730∘C2ZnO+SO2+O2ZnSO4→>1730∘C2ZnO+SO2+O2

4. Reaction with halogen:Hydrogen does not react with halogens at ordinary temperature. But at high temperature in the presence of catalyst, hydrogen react to give their respective halides.

H2+F2⟶2HFH2+F2⟶2HF

H2+Cl2⟶2HClH2+Cl2⟶2HCl

H2+Br2⟶2HBrH2+Br2⟶2HBr

H2+I2⟶2HlH2+I2⟶2Hl

Note: The reactivity order of hydrogen with other halides is: F₂ > Cl₂ > Br₂ > I₂.

Reaction with metals: It reduces metal oxides to metals, when heated.

CuO+H2−→ΔCu+H2OCuO+H2→ΔCu+H2O

ZnO+H2−→ΔZn+H2OZnO+H2→ΔZn+H2O

PbO+H2−→ΔPb+H2OPbO+H2→ΔPb+H2O

Fe2O3+4H2−→Δ3Fe+4H2OFe2O3+4H2→Δ3Fe+4H2O

 

Action with carbon monoxide: Carbon monoxide reacts with hydrogen at about 430 ^oC and 200 atmospheric pressure in the presence of ZnO and Cr₂O₃ as a catalyst to give methanol.

\ce{CO2 + 2H2->[{430^{\circ}C}][\ce{ZnO/Cr2O3}] $\underset{\text{Methanol}}{\ce{CH3OH}}\ce{CO2 + 2H2->[{430^{\circ}C}][\ce{ZnO/Cr2O3}] $\underset{\text{Methanol}}{\ce{CH3OH}}

Uses of hydrogen:

– Hydrogen is used for synthesis of ammonia in Haber’s process.
– Hydrogen is used for the manufacture of ethanol, HCl etc.
– It is used in hydrogenation of oil to produce artificial ghee.
– It is used as a reductant in metallurgical process.
– Liquid hydrogen is used as a fuel in rockets and missiles.
– It is used for filling balloons, study of atmosphere etc.