Advertisements
Advertisements
प्रश्न
Predict the product of electrolysis in the following:
An aqueous solution of AgNO3 with silver electrodes.
उत्तर
AgNO3 ionizes in aqueous solutions to form Ag+ and `"NO"_3^(-)` ions.
On electrolysis, either Ag+ ions or H2O molecules can be reduced at the cathode. But the reduction potential of Ag+ ions is higher than that of H2O.
\[\ce{Ag+_{ (aq)} + e- -> Ag_{(s)}};\] E° = + 0.80 V
\[\ce{2H_2O_{(l)} + 2e- -> H_{2(g)} + 2OH^-_{ (aq)}}\]; E° = - 0.83 V
Hence, Ag+ ions are reduced at the cathode. Similarly, Ag metal or H2O molecules can be oxidized at the anode. But the oxidation potential of Ag is higher than that of H2O molecules.
\[\ce{Ag_{(s)} -> Ag+_{(aq)} + e-}\]; E° = - 0.80 V
\[\ce{2H_2O_{(l)} -> O_{2(g)} + 4H+_{ (aq)} + 4e-}\]; E° = -1.23 V
Therefore, Ag metal gets oxidized at the anode.
APPEARS IN
संबंधित प्रश्न
Depict the galvanic cell in which the reaction Zn(s) + 2Ag+(aq) → Zn2+(aq) + 2Ag(s) takes place, further show:
- which of the electrode is negatively charged,
- the carriers of the current in the cell, and
- individual reaction at each electrode.
Predict the product of electrolysis in the following:
An aqueous solution AgNO3 with platinum 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.
