Question

Gaseous chlorine atoms would then react with gaseous ozone (`O_3`) to form gaseous chlorine monoxide and gaseous oxygen. Write the balanced chemical equation for this reaction. How do I do this?

Answer 1

I think that

`Cl_2(g)+4O_3(g)->2ClO(g)+5O_2(g)`

works

Explanation:

First, write down the unbalanced reaction.

`Cl_2(g)+O_3(g)->ClO(g)+O_2(g)`

Let's balance the chlorine first. Adding a `2` to `ClO` gives us

`Cl_2(g)+O_3(g)->2ClO(g)+O_2(g)`

Now, there are `4` oxygen atoms on the right side, and `3` on the left, so we can find their lowest common multiple, which is `12`.

So now, we want `12` oxygen atoms on both sides.

`Cl_2(g)+4O_3(g)->2ClO(g)+5O_2(g)`

Answer 2

Well, balance mass and balance charge....

Explanation:

`dotCl(g) + O_3(g)rarrClO(g) + O_2(g)`

The question specified chlorine atoms....(as opposed to garden variety `Cl_2` molecules...), and ozone molecules, which are of course a BENT triatom...`""^(-)O-stackrel(+)O=O`...the LEFT HAND oxygen as we face the page has 9 electrons (and thus a formal NEGATIVE charge). And the central oxygen atoms has 7 electrons (and thus a formal POSITIVE charge).

Of course, the neutral oxygen atom, has `Z=8`, and thus 8 electrons. And please note that I have tried to distinguish here between oxygen `"atoms"`, and dioxygen, and trioxygen molecules....dioxygen, and ozone respectively.