An aqueous solution of NaCl on electrolysis gives H2g- Cl2g and NaOH according to reaction- 2Cl-aq-2H2O- 2OH-aq-H2g-Cl2gA direct current of 25 ampere with a current efficiency of 62

The redox changes are : Anode: 2Cl^ → Cl_2+2e nbsp;Cathode : 2e+2H_2O→ 2OH^ +H_2 ...

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Chemistry

Factors Affecting Electrolysis

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Question

An aqueous solution of NaCl on electrolysis gives $H_{2}$ (g), $C l_{2}$ (g) and NaOH according to reaction,
$2 C l^{-} (a q) + 2 H_{2} O \to 2 O H^{-} (a q) + H_{2} (g) + C l_{2} (g)$
A direct current of 25 ampere with a current efficiency of 62% is passed through 20 litre of NaCl solution (20% by mass) Write down the reactions taking place at the electrodes.
The redox changes are : Cathode: $2 C l^{-} \to C l_{2} + 2 e$
Anode : $2 e + 2 H_{2} O \to 2 O H^{-} + H_{2}$

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Solution

The redox changes are : Anode: $2 C l^{-} \to C l_{2} + 2 e$ Cathode : $2 e + 2 H_{2} O \to 2 O H^{-} + H_{2}$

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An aqueous solution of NaCl on elctrolysis gives $H_{2} (g)$ , $C l_{2} (g)$ , and $N a O H$ according to the reaction

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A Direct current (DC) of 25 A with a current efficiency of 62 % is passed through 20 L of NaCl solution (20% by weight). The molarity (M) of the solution with respect to hydroxide ion will be X. The value of X is ( asssume no loss due to evaporation):

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Given are the reactions occuring during the electrolysis of sodium chloride solution:

$2 C l^{-} \to C l_{2} + 2 e^{-}$
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Which of the following is correct regarding liberation of electrolytic products?

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The redox changes are : Anode: 2Cl−→Cl2+2e Cathode : 2e+2H2O→2OH−+H2

The redox changes are : Anode: $2 C l^{-} \to C l_{2} + 2 e$ Cathode : $2 e + 2 H_{2} O \to 2 O H^{-} + H_{2}$