Advertisements
Advertisements
प्रश्न
How much electricity is required in coulomb for the oxidation of 1 mol of \[\ce{H2O}\] to \[\ce{O2}\]?
उत्तर
The electrode reaction for 1 mol of \[\ce{H2O}\] is given as –
\[\ce{H2O -> H2 + 1/2O2}\]
i.e., \[\ce{O^{2-} -> 1/2O2 + 2e^-}\]
∴ Amount of electricity required = 2 F
= 2 × 96500 C
= 193000 C
APPEARS IN
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:
An aqueous solution of \[\ce{AgNO3}\] with platinum electrodes.
Predict the product of electrolysis in the following:
A dilute solution of \[\ce{H2SO4}\] with platinum electrodes.
Predict the product of electrolysis in the following:
An aqueous solution of \[\ce{CuCl2}\] with platinum electrodes.
How much electricity is required in coulomb for the oxidation of 1 mol of \[\ce{FeO}\] to \[\ce{Fe2O3}\]?
Using the standard electrode potentials, predict if the reaction between the following is feasible:
\[\ce{Ag^+_{( aq)}}\] and \[\ce{Cu_{(s)}}\]
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:
\[\ce{Ag_{(s)}}\] and \[\ce{Fe^{3+}_{( aq)}}\]
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?
