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Electrolytic Cell

Electrolysis ...

Question

Electrolysis of an aqueous solution of $A g N O_{3}$ with silver electrodes produces $(i) - - -$ at cathode while $(i i) - -- -$ ions are dissolved from anode. When Pt electrodes are used $(i i i) - --- -$ is produced at anode and $(i v) - -- -$ at cathode.

(i)-

H_{2}

, (ii)-

N O_{3}^{-}

, (iii)-

O H^{-}

, (iv)-

H_{2}

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(i)-

A g

, (ii)-

H^{+}

, (iii)-

O_{2}

, (iv)-

H_{2}

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(i)-

A g

, (ii)-

A g^{+}

, (iii)-

O_{2}

, (iv)-

A g

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(i)-

A g

, (ii)-

H^{+}

, (iii)-

A g^{+}

, (iv)-

O_{2}

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Solution

The correct option is D (i)- $A g$ , (ii)- $A g^{+}$ , (iii)- $O_{2}$ , (iv)- $A g$
When the electrode of the same material is used for example $A g$ . The metal itself gets oxidized and reduced on an electrode.
Cathode - Reduction $A g^{+} + e^{-} ⟶ A g$
Anode - Oxidation $A g ⟶ A g^{+} + e^{-}$
When platinum electrodes are used, $A g^{+}$ from solution is reduced and deposited at cathode whereas $O_{2}$ is produced at the anode.
Cathode - Reduction $A g^{+} + e^{-} ⟶ A g$
Anode - Oxidation $2 H_{2} O ⟶ 4 H^{+} + O_{2} + 4 e^{-}$

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Similar questions

Aqueous $C u S O_{4}$ is electrolyzed using $A g$ as anode and $C u$ as cathode, then product of electrolysis at anode and cathode are, respectively

Q. Which of the following statements are correct?

(i) The electrolysis of aqueous NaCl produces hydrogen gas at the cathode and chlorine gas at the anode

(ii) 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

(iii) Oxygen and hydrogen are produced at the anode and cathode during the electrolysis of dilute aqueous solution of

H_{2} S O_{4}

(iv) All electrolytic reactions are redox reactions

Question 23
An electrolytic cell consists of:
(i) positively charged cathode.
(ii) negatively charged anode.
(iii) positively charged anode.
(iv) negatively charged cathode.

(a) (i) and (ii)
(b) (iii) and (iv)
(c) (i) and (iii)
(d) (ii) ad (iv)

Match the following:

List-I

A) Electrolysis of aq. sol. of $N a_{2} S O_{4}$ by using inert electrodes.

B) Electrolysis of 50% $H_{2} S O_{4}$ using Pt electrodes.

C) Electrolysis of Aq. sol. of $A g N O_{3}$ using inert electrodes.

D) Electrolysis of aq. $A g N O_{3}$ using silver electrodes.

List-II

1) Ag at cathode $O_{2}$ at anode

2) $H_{2}$ at cathode $O_{2}$ at anode

3) $H_{2}$ at cathode $H_{2} S_{2} O_{8}$ at anode

4) $A g^{+} + e^{-} \to A g$
$A g \to A g^{+} + e^{-}$

Question 11
Which of the following metals exist in their native state in nature?
(i) $Cu$
(ii) $Au$
(iii) $Zn$
(iv) $Ag$

(a) (i) and (ii)
(b) (ii) and (iii)
(c) (ii) and (iv)
(d) (iii) and (iv)

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Electrolysis of an aqueous solution of AgNO3 with silver electrodes produces (i)––– at cathode while (ii)–––– ions are dissolved from anode. When Pt electrodes are used (iii)––––– is produced at anode and (iv)–––– at cathode.

Electrolysis of an aqueous solution of $A g N O_{3}$ with silver electrodes produces $(i) - - -$ at cathode while $(i i) - -- -$ ions are dissolved from anode. When Pt electrodes are used $(i i i) - --- -$ is produced at anode and $(i v) - -- -$ at cathode.