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प्रश्न
Predict the product of electrolysis in the following:
An aqueous solution of AgNO3 with platinum electrodes.
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उत्तर १
At cathode: Silver ions will be reduced, and silver metal will be deposited.
At anode: The anode is not attacked, hence OH− ions have a lower discharge potential than NO3 ions. As a result, OH− ions discharge first, followed by NO3 ions, which decompose to release O2.
\[\ce{4OH -> 2H2O_{(l)} + O2_{(g)}}\]
उत्तर २
At cathode: Silver metal will be deposited as silver ions are reduced.
At anode: Water will preferentially oxidise and oxygen will evolve because its reduction potential is lower than that of \[\ce{NO^-_3}\] ions.
\[\ce{H2O_{(l)} -> \frac{1}{2} O2_{(g)} + 2H^+_{ (aq)} + 2e-}\]
संबंधित प्रश्न
Predict the product of electrolysis in the following:
An aqueous solution of \[\ce{AgNO3}\] with silver electrodes.
Predict the product of electrolysis in the following:
A dilute solution of H2SO4 with platinum electrodes.
Predict the product of electrolysis in the following:
An aqueous solution of CuCl2 with platinum electrodes.
How much electricity is required in coulomb for the oxidation of 1 mol of H2O to O2?
How much electricity is required in coulomb for the oxidation of 1 mol of FeO to Fe2O3?
Using the standard electrode potentials, predict if the reaction between the following is feasible:
\[\ce{Fe^{3+}_{ (aq)}}\] and \[\ce{I^-_{ (aq)}}\]
Using the standard electrode potentials, predict if the reaction between the following is feasible:
\[\ce{Ag^+_{ (aq)}}\] and Cu(s)
Using the standard electrode potentials, predict if the reaction between the following is feasible:
\[\ce{Fe^{3+}_{ (aq)}}\] and \[\ce{Br^-_{ (aq)}}\]
Using the standard electrode potentials, predict if the reaction between the following is feasible:
\[\ce{Br2_{(aq)}}\] and \[\ce{Fe^{2+}_{( aq)}}\]
In the following reaction, identify X:
\[\ce{Cr2O^{2-}7 + X ->[H+] Cr^{3+} + H2O + Oxidized product of X}\]
Write the reaction occurring at anode and cathode and the products of electrolysis of aq KCl.
Four half-reactions, I to IV are shown below:
- \[\ce{2Cl^- -> Cl2 + 2e^-}\]
- \[\ce{4OH^- -> O2 + 2H2O + 2e^-}\]
- \[\ce{Na^+ + e^- -> Na}\]
- \[\ce{2H^+ + 2e^- -> H2}\]
Which two of these reactions are most likely to occur when concentrated brine is electrolysed?
