 If you want to, I don't want to pressure you into being a cameraman or anything. I appreciate it. Anyway, so let's try this second one. I think we did the first one in the class today. It says, how many moles of ice at 0 degrees Celsius? So 0 degrees Celsius, that's the freezing point of ice or the melting point, right? So that's where you're going to bring in delta H fusion, right? So how many moles of ice at 0 degrees Celsius could be melted with the addition of 750 kilojoules of energy? And it says that the delta H of fusion is 6.01 kilojoules per mole. So it's asking for moles, and it gives you some information. So it says the amount of heat that they're pumping into this is 750 kilojoules of energy. And they give you delta H fusion, 6.01 kilojoules per mole. And they're wondering how many moles of ice can be melted, right? So hopefully you can see it's a simple conversion factor, right? Because we've got the conversion factor here. We're just changing from energy to number of moles, OK? And we've got the conversion factor here. So number of moles of ice in this case is going to be one mole of ice for every 6.01 kilojoules of energy. And they're nice to us. They give it to us, and they're going to kill the joules. So like that. Everybody OK with doing something like that? Simple conversion? Cancel, cancel there. We're going to have the number of moles of ice. What is it? OK, thank you. OK, so three sig figs here, right? So 125 kilojoules. OK, so that's how much? Oops, no, kilojoules. Sorry, 125 moles of ice. So that's how many moles of ice that you could melt with 750 kilojoules of energy provided the delta H of fusion was 6.01 kilojoules per mole. That makes sense? Any questions on that one? If you want to kill that one.