Sodium can be extracted by heating naturally occurring salt until it is molten. An electrochemical process is then used to extract the sodium. Cl2 is produced at the anode, and Na is collected at the cathode.
Write the half-reactions that occur at the anode and the cathode. Identify each as either oxidation or reduction. (4 points)
At the anode:
Half-reaction: 2 Cl- -> Cl2 + 2 e-
This half-reaction is an oxidation reaction.
At the cathode:
Half-reaction: 2 Na+ + 2 e- -> 2 Na
This half-reaction is a reduction reaction.
To determine the half-reactions that occur during the extraction of sodium, we need to identify the oxidation and reduction processes at the anode and cathode, respectively.
At the anode (positive electrode), chlorine gas (Cl₂) is produced. This process involves the loss of electrons and is therefore an oxidation reaction. The half-reaction at the anode can be written as:
2Cl⁻ → Cl₂ + 2e⁻
The Cl⁻ ion is oxidized to form Cl₂ gas, losing two electrons.
At the cathode (negative electrode), sodium (Na) is collected. This process involves the gain of electrons and is therefore a reduction reaction. The half-reaction at the cathode can be written as:
2Na⁺ + 2e⁻ → 2Na
The Na⁺ ions are reduced to form sodium metal by gaining two electrons.
Overall, during the extraction of sodium, the half-reactions are as follows:
At the anode (oxidation):
2Cl⁻ → Cl₂ + 2e⁻
At the cathode (reduction):
2Na⁺ + 2e⁻ → 2Na
Nn+ + e- >> Na gains electron, redkuction
3Cl- >> Cl2 + 2e= loses electrons, oxidation