Question

Two electrolytic cells containing silver nitrate & copper sulphate solution are connected in a series. The steady current of $2.5$A was passed thought them till 1.018g of silver were deposited. How long did the current flow & what is the mass of Cu deposited?

Answer 1

we have,

$A{g}^{+}+e^{-}\to Ag$

$w=\frac{E\ast I\ast t}{96500}$

$1.018=\frac{108\ast 2.5\ast t}{96500}$

$t=363.8sec$

for mass of copper deposited,

$w=\frac{E\ast I\ast t}{n\ast 96500}$

$w=\frac{63.5\ast 2.5\ast 363.8}{2\ast 96500}$

$w=0.598g$