Question

In the electrolysis of Cu(II) chloride solution using Cu electrodes the mass of the cathode is increases by 3.175g. What occurred at the copper anode?

• A. 0.112 dm${}^3$ of Cl${}_2$ was liberated
• B. 0.56 dm${}^3$ of $O_2$ was liberated
• C. 0.1 mole of Cu${}^{2+}$ passed into the solution
• D. 0.05 moles of copper is dissolved at anode

Answer 1

The correct option is D 0.05 moles of copper is dissolved at anode

In electrolysis of $CuC{l}_2$ using copper electrodes
$C{u}^{2+}$ gets oxidized at anode and $C{u}^{2+}$ from solution gets reduced at cathode
$\therefore$ mass at cathode $=3.175$
$\text{moles at cathode}=\frac{3.175}{63.75}=\frac{1}{16}$
$=0.05$