question_answer 1)

Predict the products of electrolysis in each of the following: (i) An aqueous solution of\[AgN{{O}_{3}}\] with silver electrodes. (ii) An aqueous solution of \[\text{AgN}{{\text{O}}_{\text{3}}}\]with platinum electrodes. (iii) A dilute solution of sulphuric acid using platinum electrodes. (iv) An aqueous solution of \[CuC{{l}_{2}}\] with platinum electrodes.

Answer:

(i) Anode \[Ag\to A{{g}^{+}}+{{e}^{-}}\] Cathode \[A{{g}^{+}}+{{e}^{-}}\to Ag\] (ii) Cathode \[A{{g}^{+}}+{{e}^{-}}\to Ag\] Anode \[2O{{H}^{-}}\to {{H}_{2}}O+\frac{1}{2}{{O}_{2}}+2{{e}^{-}}\] (iii) In dilute\[{{H}_{2}}S{{O}_{4}}\], electrolysis of water takes place. \[{{H}_{2}}O\rightleftharpoons {{H}^{+}}+O{{H}^{-}}\] Cathode \[2{{H}^{+}}+2{{e}^{-}}\to {{H}_{2}}\uparrow \] Anode \[2O{{H}^{+}}\to {{H}_{2}}O+\frac{1}{2}{{O}_{2}}+2{{e}^{-}}\] (iv) \[CuC{{l}_{2}}\to C{{u}^{2+}}+2{{e}^{-}}\to Cu\] Cathode \[C{{u}^{2+}}+2{{e}^{-}}\to Cu\] Anode \[2C{{l}^{-}}\to C{{l}^{2}}+2{{e}^{-}}\]