Question

A solution of $Ni(N{O}_3{)}_2$ is electrolysed between platinum electrodes using a current of $5$ amperes for $20$ minutes. What mass of $Ni$ is deposited at the cathode?

Answer 1

Given

$I=5A$

$Time=20\times 60=1200s$

$\therefore Charge=current\times time$

$=5\times 1200$

$=6000C$

According to the reaction.

$N{i}^{2+}\left(aq.\right)+2e\to Ni\left(s\right)$

$Nickeldepositeby(2\times 96487)C=58.7g$

$\therefore Nickeldepositeby6000C=\frac{58.7\times 6000}{2\times 96487}$

$=1.825g$

$\therefore$ Hence $1.825g$ of nickel will be deposited at the cathode.