 Okay, so let's try this one. But instead of reacting two moles of oxygen, let's react five moles of oxygen. Okay? See the energy that we get from reacting five moles of oxygen. And, of course, I'm gonna need my calculator to do this. This is my typical first problem experience that we're doing for my calculator. So, what does this reaction tell us? Well, this reaction is called the thermodynamic reaction equation. Okay? Because it's got some thermodynamic data. And what it's telling us here is that one of the products of this reaction is 802 kilojoules of energy. So, 802 kilojoules of energy is being released. You can think of it like the change in e is negative 802 kilojoules. Okay? Why is it negative? Because it was a product, right? And if it's a product, that means it's being released. Is everybody okay with that? Okay. So, what did we say? Instead of two moles of oxygen reacting, we've got five moles, right? 5.00, so we can have three signals. Okay? So, what is the change in energy if we've got five moles of oxygen? Well, we've got this thermodynamic data that gives us this conversion factor. Okay? Remember, stoichiometric relationships for chemical equations, balanced chemical equations. You guys recall that, right? So, in this case, we've got a stoichiometric relationship of two moles of oxygen to negative 802 kilojoules of energy. Is everybody okay with that? So, that's a conversion factor. So, effectively, what we can say is that if we want to know the energy of five moles of oxygen, well, 5.00 moles o2, moles o2 on the bottom, of course, with 802 kilojoules of energy. So, now, just five times negative o2 divided by 2. So, well, three signals, negative 2.00 times 10 to the 1, 2, 3 kilojoules of energy. Is everybody okay with that? Yes. Any questions on that one? Makes sense. Can we kill it?