What is the quantity of electricity (in Coulombs) required to deposit all the silver from $250 \mathrm{~mL}$…
What is the quantity of electricity (in Coulombs) required to deposit all the silver from $250 \mathrm{~mL}$ of $1 \mathrm{M} \mathrm{AgNO}_3$ solution?
2412.5
24125
4825.0
48250
Solution
$\begin{array}{r}
250 \mathrm{~mL} 1 \mathrm{M} \mathrm{AgNO}_3 \text { contain }=\frac{250}{1000} \\
=0.25 \mathrm{~mole}_{\mathrm{AgNO}_3}
\end{array}$
$\because \quad$ Electricity required to liberate $1 \mathrm{~g}$ equivalent of metal $=96500$ Coulomb
$\therefore$ Electricity required to liberate $0.25 \mathrm{~g}$ equivalent of metal
$=\frac{96500 \times 0.25}{1}=24125 \text { Coulomb }$