Redox problem?

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Answer 1 · 2016-12-12T17:32:48

$ClO_4^-$ , $"perchlorate ion, "Cl(VII+)$ .

$Cl_2,$ $Cl(0)$ .

$Cl^-,$ $Cl(-I)$ .

$ClO^(-),$ $"hypochlorite ion", Cl(+I)$ .

The given reaction is a redox reaction: chloride ion is oxidized to chlorine, and perchlorate is reduced to hypochlorite.

$"Oxidation (i):"$

$Cl^(-) rarr 1/2Cl_2 + e^-$

$"Reduction (ii):"$

$ClO_4^(-) +6H^(+)+ 6e^(-) rarr ClO^(-) + 3H_2O$

$"Overall": 6xx(i)+(ii):$

$6Cl^(-) +ClO_4^(-) +6H^(+)rarr 3Cl_2 + ClO^(-) + 3H_2O$