In the electrolysis of Na2SO4 solution using inert electrodea the anodic reaction is 2H2O- O2g-4e-4H-b H2g and O2g is produced in a molar ratio of 2-1c 23 grams of sodium is produced at the cathoded the cathode reaction is Na-e- Na

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Byju's Answer

Standard XII

Chemistry

Application of Electrolysis

In the electr...

Question

In the electrolysis of $N a_{2} S O_{4}$ solution using inert electrode
a) the anodic reaction is
$2 H_{2} O \to O_{2} (g) + 4 e^{-} + 4 H^{+}$
b) $H_{2} (g)$ and $O_{2} (g)$ is produced in a molar ratio of 2:1
c) 23 grams of sodium is produced at the cathode
d) the cathode reaction is $N a^{+} + e^{-} \to N a$

a and b are correct

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c,d are correct

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only c is correct

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all are correct

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Solution

The correct option is C a and b are correct
The discharge potential of $H^{+}$ ions is lower than ${N a}^{+}$ ions. Hence $H^{+}$ ions will be liberated at cathode in preference to ${N a}^{+}$ ions.
The discharge potential of ${O H}^{-}$ ions is lower than ${S O}_{4}^{2 -}$ ions. Hence ${O H}^{-}$ ions will be liberated at anode (in the form of $O_{2}$ molecule) in preference to ${S O}_{4}^{2 -}$ ions. This is the electrolysis of water. Hence $H_{2}$ and $O_{2}$ are produced in the molar ratio of 2:1 which is same as that present in water molecule.

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Similar questions

Which of the following statements are correct?

a) The electrolysis of aqueous NaCl produces hydrogen gas at the cathode and chlorine gas at the anode .

b) The electrolysis of a $C u S O_{4}$ solution using Pt electrodes causes the liberation of $O_{2}$ at the anode and the deposition of copper at the cathode .

c) Oxygen and hydrogen are produced at the anode and cathode during the electrolysis of dilute aqueous solution of $H_{2} S O_{4}$ .

d) All electrolytic reactions are redox reactions .

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O_{2} (g) + 2 H_{2} O (l) + 4 e^{-} \to 4 O H^{-} (a q)

Anode :

H_{2} (g) + 2 O H^{-} (a q) \to 2 H_{2} O (l) + 2 e^{-}

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

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Q. In a hydrogen oxygen fuel cell, electricity is produced. In this process

H_{2} (g)

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O_{2} (g)

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O_{2} (g) + 2 H_{2} O (l) + 4 e^{-} \to 4 O H^{-} (a q)

Anode :

H_{2} (g) + 2 O H^{-} (a q) \to 2 H_{2} O (l) + 2 e^{-}

4.48 L

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1 atm

and

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H_{2} (g)

is oxidised at anode and

O_{2} (g)

reduced at cathode.
Given : Cathode:

O_{2} (g) + 2 H_{2} O (l) + 4 e^{-} \to 4 O H^{-} (a q)

Anode :

H_{2} (g) + 2 O H^{-} (a q) \to 2 H_{2} O (l) + 2 e^{-}

4.48 L

H_{2}

1 atm

and

273 K

is oxidised in

9650 sec

.
The current produced is (in amp):

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In the electrolysis of Na2SO4 solution using inert electrodea) the anodic reaction is2H2O→O2(g)+4e−+4H+b)H2(g) and O2(g) is produced in a molar ratio of 2:1c) 23 grams of sodium is produced at the cathoded) the cathode reaction is Na++e−→Na