Dihydrogen

Dihydrogen is the more common name for hydrogen, which is a substance becoming the most basic of all chemical elements. Numerous applications are going to the most diverse fields of sciences and industries. It fuels rockets other than in the periodic table to send people living into orbit and on the other side of the ground, it more and more fuels clean energies. Versatility and important position in parameters regarding industry and environmental control underline the ways for its production through steam reforming of natural gas and electrolysis of water.

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This Story also Contains

1. Preparation of Dihydrogen
2. Physical Properties of Hydrogen
3. Chemical Properties of Hydrogen
4. Uses of Hydrogen
5. Ortho and Para hydrogens:
6. Some Solved Examples
7. Summary

The article will encompass all matters about him, from his production methods to his physical and chemical properties. We elaborate diatomic nature of hydrogen gas under normal conditions with high flammability and low density that decided applications in the storage of energy and fuel cells.

Rather, we see how hydrogen is involved in a range of chemical reactions from the synthesis of ammonia to refining and environmental remediation. In our exploration of hydrogen use in transportation and agriculture, we also note the curious behavior at cryogenic temperatures of ortho and parahydrogen, which manifests itself in ways that seem to depend on quantum mechanics and spectroscopy.

Join us in shedding light on the core of hydrogen in the development of our technological environment and, in the end, perhaps leading us to a future development that is sustainable and derived from the imagination and discovery of science.

Preparation of Dihydrogen

Preparation of Hydrogen: There are a number of methods for preparing dihydrogen from metals and metal hydrides.

• Laboratory Method

  • It is usually prepared by the reaction of granulated zinc with dilute hydrochloric acid.
    Zn + 2H⁺ → Zn²⁺ + H₂
  • It can also be prepared by the reaction of zinc with aqueous alkali.
    Zn + 2NaOH → Na₂ZnO₂ + H₂

• Commercial preparation method

  • The electrolysis of acidified water using platinum electrodes gives hydrogen.

    [1]
    Cathode Reaction
    2H++2e→H2

    Anode Reaction
    H2O−2e−→2H++1/2O2

    Hydrogen gas is formed at the cathode while Oxygen is formed at the anode.

    Twice as much Hydrogen as Oxygen is formed.

  • It is obtained as a byproduct in the manufacture of sodium hydroxide and chlorine by the electrolysis of brine solution. During electrolysis, the reactions that take place are:

  • At Anode: 2Cl−→Cl2+2e−
    At cathode : 2H2O(l)+2e−→H2( g)+2OH−(aq)
    Overall reaction is
    2Na+(aq)+2Cl−(aq)+2H2O(l)→Cl2(g)+H2(g)+2Na+(aq)+2OH−(aq)

  • High purity (>99.95%) dihydrogen is obtained by electrolyzing warm aqueous barium hydroxide solution between nickel electrodes.

  • By the reaction of Zn with aqueous alkali: Hydrogen can also be prepared by the reaction of zinc with aqueous alkali.

    Zn(s) Zinc +2NaOH(aq) Sodium hydroxide → Heat Na2ZnO2(aq)+H2(g)↑ Sodium zincate Hydrogen Zn(s)+ dil. 2HCl(aq) Hydrochloric acid ⟶ZnCl2(aq) Zinc chloride +H2( g)↑ (dil.)

  • Water Gas: The reaction of steam on hydrocarbons or coke at high temperatures in the presence of a catalyst yields hydrogen.

    CnH2n+2+nH2O→Ni1270 KnCO+(2n+1)H2

    The mixture of CO and H₂ is called water gas. As this mixture of CO and H₂ is used for the synthesis of methanol and a number of hydrocarbons, it is also called synthesis gas or 'syngas'.

    The process of producing 'syngas' from coal is called 'coal gasification.

    C+H2O→1270 KCO+H2

  • Water Gas Shift Reaction: The production of dihydrogen can be increased by reacting carbon monoxide of syngas mixtures with steam in the presence of iron chromate as a catalyst.

    CO(g)+H2O(g)673 K catalyst CO2( g)+H2( g)

    This is called the water-gas shift reaction.

Physical Properties of Hydrogen

Physical Properties of Hydrogen: Dihydrogen is a colorless, odorless, tasteless, combustible gas. It is lighter than air and insoluble in water. The electronegativity of hydrogen is in between metals and non-metals so it behaves as both electropositive and electronegative.

Disadvantage: A leak not only means a loss of hydrogen but is, in addition, a decided hazard because of the inflammability and very wide explosive limits that hydrogen possesses. These limits are much wider than for most gases.

The list of physical properties of Hydrogen and its isotopes are mentioned in the table below:

H-H bond Enthalpy: The H–H bond dissociation enthalpy is the highest for a single bond between two atoms of any element. It is because of this factor that the dissociation of dihydrogen into its atoms is only ~0.081% around 2000K which increases to 95.5% at 5000K. Also, it is relatively inert at room temperature due to the high H–H bond enthalpy.

Chemical Properties of Hydrogen

Chemical Properties of Dihydrogen: Dihydrogen accomplishes reactions by

(i) loss of the only electron to give H⁺

(ii) gain of an electron to form H^–

(iii) sharing electrons to form a single covalent bond.

The chemistry of dihydrogen can be illustrated by the following reactions:

• Reaction with halogens: It reacts with halogens, X₂ to give hydrogen halides, HX.

H2(g)+X2(g)→2HX(g)(X=F,Cl,Br,I)

• Reaction with dinitrogen: With dinitrogen, it forms ammonia.

3H2( g)+N2( g)→Fe673 K,200 atm2NH3( g);ΔH⊖=−92.6kjmol−1

This is the method for the manufacture of ammonia by the Haber process.

• Reaction with dioxygen: It reacts with dioxygen to form water. The reaction is highly exothermic.

2H2( g)+O2( g)→2H2O(ℓ)ΔH∘=−285.9KJ/mol

• Reactions with metals: Many metals, combine at a high temperature to yield the corresponding hydrides

  H2( g)+2M(g)→2MH(s) where M is an alkali metal

• Hydrogen reacts with many organic compounds in the presence of catalysts to give useful hydrogenated products of commercial importance. For example :

• Hydrogenation of vegetable oils using nickel as a catalyst gives edible fats (margarine and vanaspati ghee)
• Hydroformylation of olefins yields aldehydes which further undergo reduction to give alcohols.

H2+RCH2CH2CHO→RCH2CH2CH2OH

H2+CO+RCH=CH2→RCH2CH2CHO

Uses of Hydrogen

The various uses of dihydrogen are as follows:

• The largest single use of dihydrogen is in the synthesis of ammonia which is used in the manufacture of nitric acid and nitrogenous fertilizers.
• Dihydrogen is used in the manufacture of vanaspati fat by the hydrogenation of polyunsaturated vegetable oils like soybean, cotton seeds, etc.
• It is used in the manufacture of bulk organic chemicals, particularly methanol.CO(g)+2H2( g)→ coalt CH3OH(l)
• It is widely used for the manufacture of metal hydrides.
• It is used for the preparation of hydrogen chloride, a highly useful chemical.
• In metallurgical processes, it is used to reduce heavy metal oxides to metals.
• It is used as rocket fuel in space research.
• Dihydrogen is used in fuel cells for generating electrical energy. It has many advantages over conventional fossil fuels and electric power. Fuel cells generate power by establishing a potential difference between the two electrodes.
• Hydrogen produces more energy than fossil fuels.

Ortho and Para hydrogens:

In a molecule of hydrogen when the spin of both H-atoms is in the same direction, they are known as ortho hydrogen.

In a molecule of hydrogen when the spin of both H-atoms is in the opposite direction, they are known as para-hydrogen.

Recommended topic video on(Dihydrogen)

Some Solved Examples

Example 1:

Question:
Calculate the volume of hydrogen gas produced at STP when 10 grams of zinc reacts with excess dilute sulfuric acid.

Solution:
- Moles of zinc = \( \frac{10 \text{ g}}{65.38 \text{ g/mol}} = 0.153 \text{ mol} \)
- Volume of hydrogen gas at STP = \( 0.153 \text{ mol} \times 22.4 \text{ L/mol} = 3.43 \text{ L} \)

Example 2:

Question:
If 5.6 grams of water is electrolyzed using platinum electrodes, calculate the volume of oxygen gas produced at STP.

Solution:
- Moles of water = \( \frac{5.6 \text{ g}}{18.015 \text{ g/mol}} = 0.311 \text{ mol} \)
- Moles of oxygen gas = \( 0.5 \times 0.311 \text{ mol} = 0.156 \text{ mol} \)
- Volume of oxygen gas at STP = \( 0.156 \text{ mol} \times 22.4 \text{ L/mol} = 3.50 \text{ L} \)

These examples demonstrate how to calculate the volume of gases produced in chemical reactions and electrolysis experiments using simple stoichiometry and gas laws.

Summary

The importance of hydrogen goes beyond just being an element. Its influence ranges from the roots of chemistry to the most modern of applications among boundaries of science, industry, and the environment. In showing its potential, hydrogen will play a key role in moving sustainable technologies forward and overcoming global challenges.

Frequently Asked Questions
1. How is hydrogen mainly produced?
Hydrogen mainly comes from the steam reforming of natural gas and electrolysis of water where, through chemical reactions, the liberalization of hydrogen gas happens.

2. How does hydrogen contribute to clean energy?
Hydrogen fuels fuel cells in electrical vehicles and can be made from renewable resources, thus creating a clean alternative to fossil fuels.

3. What are Ortho and Para Hydrogen, and why are they important?
Ortho and Para hydrogen represent nuclear spin isomers of hydrogen that, at very low temperatures, show different properties. These properties make them very important in precise spectroscopy or when involved in cryogenic applications.

4. What are some of the significant chemical reactions of Hydrogen?
Hydrogen reacts in basic industrial processes with oxygen to form water and nitrogen to produce ammonia.

5. What are the environmental benefits of hydrogen?
Hydrogen can be derived from renewable sources and, when fed into fuel cells, will give a minimal amount of emission of greenhouse gases and thus provide a clean source of energy.