Given are the reactions occuring during the electrolysis of sodium chloride solution-2Cl- Cl2 - 2e-2H2O - 2e- H2 - 2OH-Which of the following is correct regarding liberation of electrolytic products-

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Standard X

Chemistry

Electrolysis of Aqueous Sodium Chloride

Given are the...

Question

Given are the reactions occuring during the electrolysis of sodium chloride solution:
$2 C l^{-} \to C l_{2} + 2 e^{-}$
$2 H_{2} O + 2 e^{-} \to H_{2} + 2 O H^{-}$

Which of the following is correct regarding liberation of electrolytic products?

Cathode :

N a

and

H_{2}

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Cathode :

N a

and

O_{2}

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Anode:

O_{2}

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Anode :

C l_{2}

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Solution

The correct option is D Anode : $C l_{2}$
Water plays a vital role during the electrolysis of $N a C l$ solution. Since water can be both oxidized and reduced, it competes with the dissolved $N a^{+}$ and $C l^{-}$ ions.

Having a greater tendency to get reduced than sodium ions, water gets reduced and produces hydrogen. Reduction takes place at cathode and hydrogen gas is evolved at the cathode.

Similarly, $C l^{-}$ has a greater tendency than water to get oxidised so it gets oxidised and produces chlorine gas. Oxidation takes place at anode and chlorine gas will be produced at the anode. The reactions taking place during electrolysis of $N a C l$ solution are:
At cathode: $H_{2} O (l) + 2 e^{-} \to H_{2} (g) + 2 O H^{-}$

At anode: $2 C l^{-} \to C l_{2} (g) + 2 e^{-}$

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Similar questions

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

$2 C l^{-} \to C l_{2} + 2 e^{-}$
$2 H_{2} O + 2 e^{-} \to H_{2} + 2 O H^{-}$

Which of the following is correct regarding liberation of electrolytic products?

Given that $2 C l^{-} \to C l_{2} + 2 e^{-}, E^{\circ} = - 1.36 V;$
$H_{2} O \to 2 H^{+} + \frac{1}{2} O_{2} + 2 e^{-}, E^{\circ} = - 1.23 V .$ On electrolysing 1M NaCl solution with inert electrodes, which of the following is correct regarding liberation of electrolytic products ?

Q. Consider the table of standard reduction potentials shown below.

Half-reaction	$E^{\circ}$
$C l_{2} + 2 e^{-} \to 2 C l^{-}$	$1.36 V$
$O_{2} + 4 H^{+} + 4 e^{-} \to 2 H_{2} O$	$1.23 V$
$2 H_{2} O + 2 e^{-} \to H_{2} + 2 O H^{-}$	$- 0.83 V$
$R b^{+} + e^{-} \to R b$	$- 2.93 V$

Use the information from the table and your knowledge of electrochemistry to predict the CORRECT net ionic equation for the reaction that will occur when an aqueous solution of rubidium chloride undergoes electrolysis.

Q. Consider the table of standard reduction potentials shown below.

Half-reaction	$E^{\circ}$
$C l_{2} + 2 e^{-} \to 2 C l^{-}$	$1.36 V$
$O_{2} + 4 H^{+} + 4 e^{-} \to 2 H_{2} O$	$1.23 V$
$2 H_{2} O + 2 e^{-} \to H_{2} + 2 O H^{-}$	$- 0.83$
$R b^{+} + e^{-} \to R b$	$- 2.93 V$

Use the following from the table and your knowledge of electrochemistry to predict the CORRECT net ionic equation for the reaction that will occur when a molten rubidium chloride undergoes electrolysis.

Q. 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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Given are the reactions occuring during the electrolysis of sodium chloride solution: 2Cl−→Cl2+2e− 2H2O+2e−→H2+2OH− Which of the following is correct regarding liberation of electrolytic products?

Given are the reactions occuring during the electrolysis of sodium chloride solution:
$2 C l^{-} \to C l_{2} + 2 e^{-}$
$2 H_{2} O + 2 e^{-} \to H_{2} + 2 O H^{-}$

Which of the following is correct regarding liberation of electrolytic products?