 Okay, so last problem of the day, balance the reaction between solid tan and this aqueous solution, okay, to produce the following products. Okay, so again the first thing we need to do is to figure out which thing got oxidized and which thing got reduced. Okay, so hopefully you can see that tan went from a zero state to something that was. So tan zero goes to 10 something plus some electrons, right? So how do we figure out what the oxidation state of 10 is over here? Do what we've been doing, right, in the last other problem. Okay, so SNCl6 2 minus, right? So the whole thing is going to help me out, 2 Cl minus 1 plus X, right, like that. So X minus 6 equals minus 2. So you put an A instead of a 2. Oh, sorry. 2, right, so when we move that over it's going to be plus 4, okay? Everybody's cool with that? Yes. If I can do my math right, that would be easier for me, but I won't be confused. Okay, so we can put that whole thing in there, but for me it's easier to just look at the tan by itself, okay? So I'm just going to put a tan 4 plus like that. Everybody okay with that? And so when we do that, 4 electrons. Is that okay? So that's one of the half reactions. Oxidation or reduction? Oxidation. Oxidation should be faster than that. Okay, so right, what did we say? Was the NO3 minus that's getting reduced, the nitrogen, plus some amount of electrons goes to NO2, right? Everybody's saying that that's the one. Okay, so I'd like to keep it like this, even though the oxygens will not be balanced, okay? It's not going to be balanced. So how do we figure this out? What's the oxidation number of nitrogen here? Plus 4. What's the oxidation number of nitrogen here? 3. Plus 5. 1, right? So is that the same as that? This half reaction. Multiply it by 4, okay? Is everybody okay with what we're doing? Have we transferred the right amount of electrons? Okay, remember I told you your oxygens won't be balanced at this point in time, okay? Is everybody okay with that? Now let's just put those numbers in. So NO3 minus 4 there, NO2, 4 there. That lets your reaction. So let's see if I can do this. So what do we got? 3 times 4 oxygens, right? So that's 12 oxygens here. On this side, we've got 2 times 4, which is 8, right? So plus this over here. So we're going to need 4 more, right? From here. So 4, like that. 4 plus 8 is 12, right? That's cool with oxygens. Okay, so now we've got hydrogens over here, but not as many over here. So we've got to balance that, right? So 4 times 2 is 8, how many? Okay, we're going to go fast. 8 is because the fling's flashing. So have we balanced it? No, chlorine still needs to balance, right? 6. Can we balance everything? I think it's balanced. That's your balanced reaction, okay? So do you guys see how to do it? Okay, so remember, have reactions first and then multiply by the factor and then balance your reaction, okay? Sorry guys, I have to go fast because the thing's going to die, okay? Bye-bye.