* Potassium metal (K) at the cathode (negative electrode)
* Chlorine gas (Cl₂) at the anode (positive electrode)
Here's a breakdown of the process:
At the cathode:
* K⁺ ions from the molten KCl are attracted to the negatively charged cathode.
* They gain electrons and are reduced to potassium metal:
K⁺ + e⁻ → K
At the anode:
* Cl⁻ ions from the molten KCl are attracted to the positively charged anode.
* They lose electrons and are oxidized to chlorine gas:
2Cl⁻ → Cl₂ + 2e⁻
Overall reaction:
2KCl(l) → 2K(l) + Cl₂(g)
It's important to note that electrolysis of molten potassium chloride requires a high temperature to melt the salt and facilitate the movement of ions.
