Predict the products of electrolysis in each of the following:
(i) An aqueous solution of AgNO₃ with silver electrodes.
(ii) An aqueous solution of AgNO₃ with platinum electrodes.
(iii) A dilute solution of H₂SO₄ with platinum electrodes.
(iv) An aqueous solution of CuCl₂ with platinum electrodes.

At cathode: Ag⁺ are preferably discharged as compared to H⁺ as its reduction potential is higher

Ag to the power of plus plus straight e to the power of minus space rightwards arrow space Ag left parenthesis straight s right parenthesis

At anode: Silver electrode (being reactive) dissolves to produce Ag⁺As the electrodes are inert, these do not take part in the reaction. At cathode, Ag⁺ ions are discharged in preference to H⁺ ions and OH^– are discharged in preference to NO₃^– ions at anode
At cathode: Ag+ are preferably discharged as compared to H+ as its

At cathode: Ag+ are preferably discharged as compared to H+ as its

Here, only H⁺ are discharged at cathode as there is no other positive ion. Out of OH^– and SO₄^2– ions, OH^– ions are discharged at anode preferably
At cathode: Ag+ are preferably discharged as compared to H+ as its

The platinum electrodes are inert and do not take part in the reaction. The following reactions occur at platinum (inert) electrodes.
At cathode: Ag+ are preferably discharged as compared to H+ as its

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