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#