Balancing Complete Redox Reactions
I need help on the half reduction part for both reduction and oxidation of
Cl2(g) --> cl^1- (aq) + OCl^1- (aq). I got both of the half reactions started. Cl2 --> Cl^- (Reduction) .... Cl^1- (aq) + OCl^1- (aq) (Oxidation)
See your other posts.
To balance the half-reduction reactions for Cl2(g) → Cl^1- (aq) and Cl^1- (aq) + OCl^1- (aq), you'll need to follow a few steps. Let's start with the half-reduction reaction for Cl2 → Cl^-.
1. Write the unbalanced half-reduction equation: Cl2 → Cl^-
2. Assign oxidation states to each element: Cl2 (0) → Cl^- (-1)
3. Balance the non-oxygen and non-hydrogen elements: Cl2 → 2Cl^-
4. Balance the charges: Cl2 + 2e^- → 2Cl^-
Now, let's move on to the half-oxidation reaction for Cl^- + OCl^-.
1. Write the unbalanced half-oxidation equation: Cl^- + OCl^- →
2. Assign oxidation states to each element: Cl^- (-1) + OCl^-
(oxidation state of Cl = -1, oxidation state of O = -2)
3. Balance the non-oxygen and non-hydrogen elements: Cl^- + OCl^- → Cl^- + ClO^- (the oxygen is balanced)
4. Balance the charges: Cl^- + OCl^- + e^- → Cl^- + ClO^-
Finally, to complete the balanced equation, combine the two half-reactions:
Cl2 + 2e^- → 2Cl^- (multiply the reduction half-reaction by 2)
Cl^- + OCl^- + e^- → Cl^- + ClO^- (cancel out the Cl^-)
The balanced equation becomes:
Cl2 + 2Cl^- + 2OH^- → 2Cl^- + ClO^- + H2O