 We want exactly like what we did on our lab. Yes, so you guys are good with that. Yeah, so we have the work. OK, yeah, sure. So suppose a student starts with one gram of an unknown copper compound and isolates 0.9794 grams of metallic copper. If there's only one copper atom per unit formula, what would be the formula weight of the compound? And does this result make sense? So recall what we're doing. We're doing, well, we're isolating copper from copper 2 plus ions in solution. And we're reacting them with magnesium metal. And then that's going to go to solid copper coming out of solution plus magnesium 2 plus ion. So hopefully, I don't have to break this up into two half reactions. You can see that it's two electrons and two electrons. OK, so the mass initial is going to be 1.000 grams of the unknown copper compound. And it says that it isolates some sort of mass of copper. So 0.9794 grams of copper. OK, so the thing you're going to have to do is figure out the number of moles of copper. So how do we do that? Well, we look at our periodic table and it tells us that copper is 63.55 grams per mole. That's the number of moles of copper that we got. Well, we don't know what the compound is, but we know that there's only one copper atom per unit formula. And this is the mass of the compound. So in order to figure out, well, so what is it saying? So it's 1 mole of Cu per 1 mole of the compound. Everybody's cool with that, right? Because there's only one copper per. Let's just do that conversion just so everybody's on the same page. The number of moles, and we know the mass, right? So molar mass is what? Grams per mole. So in order to find the molar mass or formula weight, if you want to think of it that way, essentially the same thing. We'll find the formula weight in a second. Of the compound, we've got to figure out the molar mass first. So 0.01541 moles of the compound divided by 1.000 grams of the compound on the compound. So grams per mole, that's molar mass. So that's 64 point weight would be 64.89 AMU. So very similar. So the formula weight is what it's asking for. So formula weight of the compound, 64.89 Dalton's or AMU or whatever you want to say. And does this result make sense? Well, to me, no, it doesn't make very much sense. Why is that? Because copper is 63.55 grams or AMUs, right? So what am I saying in here? So the mass of the compound that's not copper, let's figure that out. So mass that's unknown, unknown. So it's going to be 64.89 AMU minus 63.55 AMU. And when we do that, we get 1.337 AMU. So the compound would be copper plus something else that is only this mass. And that's like 1 and 1 third hydrogen atoms. And that doesn't make any sense. So what are they saying? This person who did this experiment probably mucked up somewhere. Is that cool with everybody? So I think the important part was to do this grams per mole, to figure out the molar mass, just to remind ourselves that we can do that if we know that this is pure compound. Everybody cool? So we'll call it a night with that. Question? How do you know? Because that's what we're doing. Well, that is the action that we did is because that's the experiment that we were doing. OK, yeah, I didn't specify. I was kind of confused. Yeah, I didn't specify. I'll specify it. OK. Questions on this problem or?