Question

What is oxidation and reduction in electrolysis?

Answer 1

1. Electrolysis is the process where we apply electric current for a chemical change in a reaction.
2. This reaction occurs at electrodes that are Anode (positive electrode) and Cathode (negative electrode).
3. The cathode acts as an oxidizing agent and the gain of electrons takes place at the cathode, this means that reduction occurs at Cathode.
4. The anode acts as a reducing agent and the loss of electrons takes place at the anode which means that oxidation occurs at the anode.
5. An example of Redox in electrolysis is When Zinc $\left(\mathrm{Zn}\right)$is reacted with Copper sulfate $\left({\mathrm{CuSO}}_4\right)$it forms Copper $\left(\mathrm{Cu}\right)$ and Zinc sulfate$\left({\mathrm{ZnSO}}_4\right)$.
   $\mathrm{Zn}\left(\mathrm{s}\right)+{\mathrm{CuSO}}_4\left(\mathrm{aq}\right)\to {\mathrm{ZnSO}}_4\left(\mathrm{aq}\right)+\mathrm{Cu}\left(\mathrm{s}\right)$
6. At the Zinc, anode oxidation occurs and the oxidation half-reaction is
   $\mathrm{Zn}\left(\mathrm{s}\right)\to {\mathrm{Zn}}^{2+}+2{\mathrm{e}}^{-}$
7. At Copper, cathode reduction takes place and the half-reaction reaction is
   ${\mathrm{Cu}}^{2+}+2{\mathrm{e}}^{-}\to \mathrm{Cu}\left(\mathrm{s}\right)$