Balance the chemical equation for the following redox reaction under acidic aqueous conditions with the smallest whole-number coefficients possible using the half-reaction method.On which side does H₂O(l)appear,and what is its coefficient? Te(s)+ ClO₃^-(aq)$\to$H₆TeO₆(aq)+ Cl₂(g)

Question

Quizplus · Accepted Answer

First, we need to split the equation into two half-reactions:

Te(s) --> TeO32-(aq) (oxidation half-reaction)

ClO3-(aq) + 6H+(aq) + 6e- --> Cl-(g) + 3H2O(l) (reduction half-reaction)

Balance the number of electrons transferred by multiplying the oxidation half-reaction by 6 and the reduction half-reaction by 2:

6Te(s) + 15H2O(l) + 6ClO3-(aq) --> 6TeO32-(aq) + 6Cl-(g) + 30H+(aq)

This shows that HS- ion appears on the left side of the equation with a coefficient of 12.

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