Question
Discuss the manufacture of chlorine.
✓
Answer
Electrolytic process:
When a solution of brine $( NaCl )$ is electrolysed, $Na +$ and $CP$ ions are formed. $Na ^{+}$ion reacts with $OH ^{-}$ions of water and forms sodium hydroxide. Hydrogen and chlorine are liberated as gases.
$
\begin{array}{lll}
NaCl \longrightarrow Na ^{+}+ Cl _{\text { }}^{-} & \text {At the cathode, } & \text { At the cathode, } \\
H _2 O \longrightarrow H ^{+}+ OH ^{-} & H ^{+}+ e ^{-} \longrightarrow H & Cl ^{-} \longrightarrow Cl + e ^{-} \\
Na ^{+}+ OH ^{-} \longrightarrow NaOH & H + H \longrightarrow H _2 & Cl + Cl \longrightarrow Cl _2
\end{array}
$
Deacons process:
In this process a mixture of air and hydrochloric acid is passed up a chamber containing a number of shelves, pumice stones soaked in cuprous chloride are placed. Hot gases at about 723 $K$ are passed through a jacket that surrounds the chamber.
$
4 HCl + O _2 \underset{ Cu _2 Cl _2}{\stackrel{40{ }^{\circ} C }{\longrightarrow}} 2 H _2 O + Cl _2 \uparrow \text { }
$
When a solution of brine $( NaCl )$ is electrolysed, $Na +$ and $CP$ ions are formed. $Na ^{+}$ion reacts with $OH ^{-}$ions of water and forms sodium hydroxide. Hydrogen and chlorine are liberated as gases.
$
\begin{array}{lll}
NaCl \longrightarrow Na ^{+}+ Cl _{\text { }}^{-} & \text {At the cathode, } & \text { At the cathode, } \\
H _2 O \longrightarrow H ^{+}+ OH ^{-} & H ^{+}+ e ^{-} \longrightarrow H & Cl ^{-} \longrightarrow Cl + e ^{-} \\
Na ^{+}+ OH ^{-} \longrightarrow NaOH & H + H \longrightarrow H _2 & Cl + Cl \longrightarrow Cl _2
\end{array}
$
Deacons process:
In this process a mixture of air and hydrochloric acid is passed up a chamber containing a number of shelves, pumice stones soaked in cuprous chloride are placed. Hot gases at about 723 $K$ are passed through a jacket that surrounds the chamber.
$
4 HCl + O _2 \underset{ Cu _2 Cl _2}{\stackrel{40{ }^{\circ} C }{\longrightarrow}} 2 H _2 O + Cl _2 \uparrow \text { }
$
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