Question

Complete and balance the following redox equation using the set of smallest whole-number coefficients. Now sum the coefficients of all species in the balanced equation. (Remember the coefficients that are equal to one.) BrO3-(aq) + Sb3+(aq) ? Br-(aq) + Sb5+(aq) (acid solution) The sum of the coefficients is ___.

Answer 1

Answer:

17

Explanation:

Oxidation reaction is defined as the chemical reaction in which an atom looses its electrons. The oxidation number of the atom gets increased during this reaction.

$X\rightarrow X^{n+}+ne^-$

Reduction reaction is defined as the chemical reaction in which an atom gains electrons. The oxidation number of the atom gets reduced during this reaction.

$X^{n+}+ne^-\rightarrow X$

For the given chemical reaction:

$BrO_3^-(s)+Sb^{3+}(aq.)\rightarrow Br^-(aq.)+5Sb^{5+}(aq)$

The half cell reactions for the above reaction follows:

Reduction half reaction:  $BrO_3^-+6H^++6e^-\rightarrow Br^{-}+3H_2O$

Oxidation half reaction:  $Sb^{3+}\rightarrow Sb^{5+}+2e^-$

Multiplying the Oxidation half reaction by 3 and we get that:-

$3Sb^{3+}\rightarrow 3Sb^{5+}+6e^-$

Adding the half reactions, we get that:-

$BrO_3^-+6H^++3Sb^{3+}\rightarrow Br^{-}+3Sb^{5+}+3H_2O$

The sum of the coefficients is:- 1 + 6 + 3 + 1 + 3 + 3 = 17