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Dihydrogen - Practice Questions & MCQ

Edited By admin | Updated on Sep 18, 2023 18:35 AM | #JEE Main

Quick Facts

Preparation of Dihydrogen is considered one the most difficult concept.
Uses of Hydrogen is considered one of the most asked concept.
25 Questions around this concept.

Solve by difficulty

EASY

$\mathrm{Zn}+2 \mathrm{NaOH} \rightarrow A+B$

A could be :

ZnO

NaH

Na2ZnO2

1 and 2

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Which of the given compounds can enhance the efficiency of hydrogen storage tank?

$\mathrm{Di-isobutyl\; aluminium \; hydride}$

$\mathrm{NaNi}_5$

$\mathrm{Li} / \mathrm{P}_4$

$\mathrm{SiH}_4$

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Concepts Covered - 0

Preparation of Dihydrogen

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

Laborartory 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.
- 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:
- $At \;Anode:2Cl^{-}\rightarrow Cl_{2}+2e^{-}$
  
  $At \:cathode:2H_{2}O(l)+2e^{-}\rightarrow H_{2}(g)+2OH^{-}(aq)$
  
  $Overall \;reaction\;is$
  
  $2Na^{+}(aq)+2Cl^{-}(aq)+2H_{2}O(l)\rightarrow Cl_{2}(g)+H_{2}(g)+2Na^{+}(aq)+2OH_{-}(aq)$
- 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.
- Water Gas : Reaction of steam on hydrocarbons or coke at high temperatures in the presence of catalyst yields hydrogen.
  
  $C_{n}H_{2n+2}+nH_{2}O\xrightarrow[Ni]{1270K}nCO+(2n+1)H_{2}$
  
  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.
  
  $C+H_{2}O\overset{1270K}{\rightarrow}CO+H_{2}$
- 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 catalyst.
  
  $CO(g)+H_2O(g) \xrightarrow[catalyst]{673K}CO_2(g)+H_2(g)$
  
  This is called water-gas shift reaction.

Physical Properties of Hydrogen

Physical Properties of Hydrogen: Dihydrogen is a colourless, odourless, 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, $X_2$ to give hydrogen halides, $HX$ .

$H_{2}(g)+X_{2}(g)\rightarrow 2HX(g) \;\;(X=F,Cl,Br,I)$

Reaction with dinitrogen: With dinitrogen it forms ammonia.

$3H_2(g)+N_2(g)\xrightarrow[Fe]{673K, 200atm}2NH_3(g);$ $\Delta H^\circleddash =-92.6\; kj\;mol^{-1}$

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.

$2 \mathrm{H}_{2}(\mathrm{g})+\mathrm{O}_{2}(\mathrm{g}) \rightarrow 2 \mathrm{H}_{2} \mathrm{O}(\mathrm{\ell})$ $\Delta H^{\circ}=-285.9 \;KJ/mol$

Reactions with metals: With many metals it combines at a high temperature to yield the corresponding hydrides

$H_{2}(g)+2M(g)\rightarrow 2MH(s)\;where\;M\;is\;an\;alkali\;metal$
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 catalyst gives edible fats (margarine and vanaspati ghee)
Hydroformylation of olefins yields aldehydes which further undergo reduction to give alcohols.

$H_{2}+ RCH_{2}CH_{2}CHO\rightarrow RCH_{2}CH_{2}CH_{2}OH$

$H_{2}+CO+RCH=CH_{2}\rightarrow RCH_{2}CH_{2}CHO$

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.
$\mathrm{CO}(\mathrm{g})+2 \mathrm{H}_{2}(\mathrm{g}) \overset{\mathrm{cobalt}}{\rightarrow}\mathrm{CH}_{3} \mathrm{OH}(\mathrm{l})$
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 fuel.