# When sodium chlorate (I), NaClO is heated, sodium chlorate (V) and sodium chloride are formed. What is the ionic equation for this reaction? What type of reaction is this?

Dec 9, 2017

This is a $\text{disproportionation reaction}$, in which chlorine is $\text{OXIDIZED}$ and $\text{REDUCED...}$

#### Explanation:

$\text{Oxidation:}$
$\stackrel{{I}^{+}}{C} l {O}^{-} + 2 {H}_{2} O \rightarrow \stackrel{{V}^{+}}{C} l {O}_{3}^{-} + 4 {H}^{+} + 4 {e}^{-}$ $\left(i\right)$

$\text{Reduction:}$
stackrel(I^+)ClO^(-) + 2H^+ + 2e^(-) rarr stackrel(""^(-)I)Cl^(-)+H_2O $\left(i i\right)$

And so we takes....$\left(i\right) + 2 \times \left(i i\right)$

stackrel(I^+)ClO^(-) +2stackrel(I^+)ClO^(-) cancel(+2H_2O+ 4H^+ + 4e^(-))rarr stackrel(V^+)ClO_3^(-)+2stackrel(""^(-)I)Cl^(-)cancel(+4H^+ +2H_2O+4e^(-))

...to give....after cancellation....

stackrel(I^+)ClO^(-) +2stackrel(I^+)ClO^(-) rarr stackrel(V^+)ClO_3^(-)+2stackrel(""^(-)I)Cl^(-)

Chlorine is simultaneously reduced and oxidized....i.e. a $\text{disproportionation...}$

Is this balanced with respect to mass and charge? Don't trust my 'rithmetic....