Law of chemical equivalence

In this reaction,  

$$\ce{KIO\_3 + KI -> I\_2}$$ 
According to law of chemical equivalence, shouldn't $m\_{eq}$ of $\ce{KIO\_3}$ = $m\_{eq}$ of $\ce{KI}$ = $m\_{eq}$ of $\ce{I\_2}$?  

However, the book that I was reading from, said:  

Total $m\_{eq}$. of $\ce{I\_2}$ = $m\_{eq}$ of $\ce{I\_2}$ (from $\ce{KIO\_3}$) + $m\_{eq}$ of $\ce{I\_2}$ (from $\ce{KI}$).  

Why is it so?




This Reaction is a Disproportionation Reaction, that is, a reaction involving both oxidation and reduction of a single species, in this case : Iodine. This is not one reaction but a combination of two reactions:
$$\ce{KIO3 -> I2}$$
And
$$\ce{KI -> I2}$$
Therefore, by applying law of chemical equivalence in both reactions and adding the equations :


$m\_{eq}$ of $\ce{I\_2}$ (from both reactions) = $m\_{eq}$ of $\ce{I\_2}$ (from $\ce{KIO3}$) + $m\_{eq}$ of $\ce{I\_2}$ (from $\ce{KI}$) 


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