Chemistry - Electrochemistry Question with Solution | TestHub

The chemical equation for deposition of silver from the salt solution is

${\mathrm{Ag}}^{+}\left(\mathrm{aq}\right)+{\mathrm{e}}^{-}\stackrel{}{\to }\mathrm{Ag}\left(\mathrm{s}\right)$

Clearly, for deposition of one mole of silver one-mole electrons are required.

• Charge on one mole of the electron is equal to one Faraday or $96500$ Coulombs.
• The mass of one mole of silver is equal to its molar mass, i.e., $108 \mathrm{g}$.

Thus, we can say that

$96500$ coulomb charge can deposit $108 \mathrm{g}$ of silver.

Therefore, $965$ coulomb will deposit $\frac{108}{96500}\times 965=1.08 \mathrm{g}$ of silver.