How do I separate this redox equation into 2 half-reactions: in basic sol Cl2(g) ----> Cl-(aq) + OCl-(aq) ?
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I know the steps to solve balancing a redox equation in a basic solution, but I can't figure out what the two half-reactions are for this equation. Help please!
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Answer:
Chlorine is being oxidized and reduced!! This is a disproportionation reaction common to the halogens. 4 OH-(aq) + Cl2(g) ----------> 2 ClO-(aq) + 2 e- + 2 H2O Cl2(g) + 2 e- ---------> 2 Cl-(aq) 2 Cl2(g) + 4 OH-(aq) ---------> 2 H2O + 2 Cl-(aq) + 2 ClO-(aq)
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