Preparation of Hydrogen

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Laboratory Preparation of Hydrogen
- Action of Dilute Acid on Zinc or Iron
- Action of Sodium Metals on Cold Water
- Action of Iron on steam
Industrial Preparation of Hydrogen
- From Water Gas (Bosch Process)
- From Natural Gas and Hydrocarbon
- Incomplete Oxidation of Hydrocarbons
- Reduction of Steam with CO
- By Electrolytic Methods

When certain metals react with dilute mineral acids, water or steam, hydrogen is liberated in the process. Hydrogen is also liberated when zinc (Zn), tin (Sn) or aluminium (Al) reacts with hot concentrated solutions of sodium or potassium.

For example:

\( \scriptsize Sn + 2NaOH + 4H_2O \rightarrow Na_2(Sn(OH)_6) + 2H_2 \)

Laboratory Preparation of Hydrogen:

Hydrogen is prepared in the laboratory by the:

1. Action of Dilute Acid on Zinc or Iron:

Dilute hydrochloric acid or tetraoxosulphate(VI) acids liberate hydrogen gas with zinc or iron. The gas is collected over water since it is relatively insoluble in water and lighter than air. To dry the gas, the gas is passed over fused calcium chloride.

Zn(s) + H₂SO_4(aq) → ZnSO_4(aq) + H_2(g)

Zn(s) + 2HCl_(aq) → ZnCl_2(aq) + H_2(g)

Preparation of Hydrogen 4 — _{Hydrogen is prepared in the laboratory by the action of dilute acid on zinc or iron.}

Dilute trioxonitrate(V) acid is strongly oxidizing in nature and so it is not used for the preparation of hydrogen gas. However, it produces hydrogen gas with magnesium metal only.

2. Action of Sodium Metals on Cold Water:

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SS2: CHEMISTRY - 3RD TERM

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