Hydrogen
1.0 Basic Information
2.0 Atomic and Physical Properties of Hydrogen (reference: NCERT)
3.0 Dihydrogen
4.0 Physical Properties
5.0 Chemical Properties
6.0 Uses of Dihydrogen
7.0 Compounds of Hydrogen
8.0 Hard and Soft Water
9.0 Hydrogen Peroxide
10.0 Volume strength of Hydrogen Peroxide
8.1 Preparation
1. Electrolysis of acidified water using platinum electrodes gives hydrogen.
$$2{H_2}O\left( l \right)\mathop \to \limits_{Traces{\text{ }}of{\text{ }}acid/base}^{Electrolysis} 2{H_2}\left( g \right) + {O_2}\left( g \right)$$
2. It is usually prepared by the reaction of granulated zinc with dilute hydrochloric acid.
$$Zn + 2{H^ + } \to Z{n^{2 + }} + {H_2}$$
3. High purity ($>99.95\%$) dihydrogen is obtained by electrolysing warm aqueous barium hydroxide solution between nickel electrodes.
4. Hydrogen can be obtained by reaction of metals like $Zn$, $Al$, $Be$ etc. with alkalies.
$$\begin{equation} \begin{aligned} Zn + 2NaOH \to N{a_2}Zn{O_2} (\text{Sodium zincate})+ {H_2}\end{aligned} \end{equation} $$$$\begin{equation} \begin{aligned} Be + 2NaOH \to N{a_2}Be{O_2} (\text{Sodium beryliate})+ {H_2} \end{aligned} \end{equation} $$
5. 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:
$$\begin{equation} \begin{aligned} {\text{At Anode: }}2C{l^ - }\left( {aq} \right) \to C{l_2}\left( g \right) + 2{e^ - } \\ {\text{At cathode: }}2{H_2}O\left( l \right) + 2{e^ - } \to {H_2}\left( g \right) + 2O{H^ - } \\ {\text{The overall reaction is:}} \\ 2N{a^ + }\left( {aq} \right) + 2C{l^ - }\left( {aq} \right) + 2{H_2}O\left( l \right) \to C{l_2}\left( g \right) + {H_2}\left( g \right) + 2N{a^ + }\left( {aq} \right) + 2O{H^ - }\left( {aq} \right) \\\end{aligned} \end{equation} $$
6. Lane’s Process:
$$3Fe + 4{H_2}O\mathop \to \limits^\Delta F{e_3}{O_4} + 4{H_2}$$
7. Dihydrogen can be prepared by action of water or dilute mineral acid on metals.
$$2N{a^ + }\left( s \right) + 2{H_2}O\left( l \right) \to 2NaOH\left( {aq} \right) + {H_2} \uparrow $$ This reaction is vigorous. To minimize the rate of reaction, alkali metals are used in the form of amalgams (alloys of metal with $Hg$).
$$2Na\left( {Hg} \right) + 2{H_2}O \to 2NaOH + {H_2} \uparrow + 2Hg$$
8. Bosch Process:
Reaction of steam on hydrocarbons or coke at high temperatures in the presence of catalyst yield hydrogen.
$${C_n}{H_{2n + 2}} + n{H_2}O\mathop \to \limits_{Catalyst}^{1270K} nCO + \left( {2n + 1} \right){H_2}$$
The mixture of $CO$ and $H_{2}$ is called water gas. As this mixture of $CO$ and $H_{2}$ is used for the synthesis of methanol and a number of hydrocarbons, it is also called synthesis gas or 'syngas'. Nowadays 'syngas' is produced from sewage, saw-dust, scrap wood, newspapers etc. The process of producing 'syngas' from coal is called 'coal gasification'.