How do you write a balanced equation for this redox reaction using the smallest whole number coefficients?

The reaction occurs in aqueous acidic solution.

#"ClO"^(-)+"I"_2->"Cl"^(-)+"IO"_3^-#

1 Answer
Sep 27, 2017

Answer:

Well try.....

#I_2 + 5ClO^(-) +H_2O rarr 2IO_3^(-) +5Cl^(-) +2H^(+) #

Explanation:

Hypochlorite is REDUCED.....#stackrel(+I)Clrarrstackrel(-I)Cl#

#ClO^(-) + 2H^+ + 2e^(-) rarr Cl^(-) +H_2O# #(i)#

Charge and mass are balanced, so tick.....

And elemental iodine is oxidized.....#stackrel(0)I_2rarrstackrel(+V)I#

#1/2I_2 + 3H_2O rarr IO_3^(-) +6H^(+) + 5e^(-)# #(ii)#

Charge and mass are balanced, so double tick.....

And so we take #5xx(i)+2xx(ii)#.........

#I_2 + 5ClO^(-) +H_2O rarr 2IO_3^(-) +5Cl^(-) +2H^(+) #

Is this balanced with respect to mass and charge? If it is not, then we may reject it out of hand!