More than one way of balancing a chemical equation My textbook had this question on balancing chemical reactions 


  Ozone reacts with nitric oxide to give nitrogen dioxide and oxygen gas


Here's how I balanced it: $$\ce{O3 + NO -&gt; NO2 + O2}$$

However I realised that the equation is also balanced if I write it as: $$\ce{2O3 + 4NO -&gt; 4NO2 + O2}$$

and when it is written as: $$\ce{3O3 + NO -&gt; NO2 + 4O2}$$

This seems wrong as I am sure that there cannot be more than one way of balancing a reaction but I do not have a satisfactory explanation. What is going wrong here?
This happens when you have a sum of two (or more) independent reactions. You can balance each one, and then add them together in an arbitrary proportion. People usually run into this when trying to come up with an equation for combustion of gunpowder, where the oxidation of carbon and oxidation of sulfur are pretty much independent.

Now, in your case the reactions are:
$$\ce{2O3 -&gt; 3O2}\tag A$$
and
$$\ce{2NO + O2 -&gt; 2NO2}\tag B$$
Your first reaction is a combination of ${1\over2}A+{1\over2}B$, the second is $A+2B$, and the third is ${3\over2}A+{1\over2}B$. There are infinitely many possible combinations.

Ozone, being an extremely powerful oxidant, is known to participate in certain reactions where it spends one atom of oxygen and the rest falls off as the less reactive $\ce {O2}$, but this is not the case here. $\ce {O2}$ reacts with $\ce {NO}$ instantly, as well as $\ce {O3}$.