Now I get to manganese chloride and

I'm going to say again that manganese is going to be equal to some value y.

I need a variable there plus 2 times the oxidation state of

chlorine here which is minus1.

And that's going to be equal to 0.

And so I get that y equals 2.

So now my oxidation state in the product side for

mang, manganese is plus 2, for chlorine is minus 1.

Here I have Cl2 as a free element inside the oxidation state is going to be 0.

For hydrogen it's plus 1 and oxygen it's minus 2.

So now what I want to look for is what species are changing oxidation states.

And I see that manganese goes from plus 4 to plus 2.

And I see that chlorine, while some of it stays the same,

I also see that some chlorine goes from minus 1 to 0.

So when I look at the manganese going from plus 4 to plus 2.

That's happening because of a gain of electrons and

as a result this is the reduction process.

So it's the manganese that is being reduced or

the manganese oxide that's being reduced.

When I look at my chlorine going from minus 1 to an oxidation state of 0.

What I see happening there is the loss of electrons because I'm

becoming more positive in the oxidation state.

And so that is going to be my oxidation process.

So the HCL is oxidized to CL2.