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?

2 Answers
Jan 17, 2018

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)#

Jan 17, 2018

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.