Question

An electrolytic cell is composed of $Cu$ and $Zn$. A current of $9.65A$ is drawn from a cell for $1$ hour. Then the loss in mass at anode and gain in mass at cathode, respectively could be:

• A. $11.77g,11.43g$
• B. $11.77g,10g$
• C. $22.86g,23.54g$
• D. $23.54g,22.86g$

Answer 1

The correct option is A $11.77g,11.43g$

$W=\frac{I\times t\times M}{nF}$

$I\to$ current

$t\to$ time

$W\to$ weight deposited

$M\to$ Molar mass

$n\to$ No. of electrons involved

$F\to$ faraday's constant$=96500$

For Copper $\left(Cu\right)$

$M=63.5$g/mol

$n=2$

$I=9.65$A

$t=1$hr $=3600$sec

$W=\frac{9.65\times 3600\times 63.5}{2\times 96500}W=11.43g$

For Zinc $\left(Zn\right)$

$M=65.38$g/mol

$n=2$

$W=\frac{9.65\times 3600\times 65.38}{2\times 96500}=11.77g$