 So it says when 25 mils of 1.0 molar sulfuric acid is added to 50 mils of 1.0 molar sodium hydroxide at 25 degrees Celsius and a calorimeter, the temperature of the aqueous solution increases to 33.9 degrees Celsius. Assuming that the specific heat of the solution is 4.18 joules per grams to degrees Celsius, that the density is 1.00 grams per mil and that the calorimeter itself absorbs no amount of heat, calculate the delta heat of reaction in kilojoules for this reaction. Is the energy being gained or lost by the system? And the other thing we have to imagine is that the volumes are strictly added, OK? So if you guys don't understand what that means, it's OK. But anyways, so let's write down the things that we know that it gives. So it gave us the initial temperature. So Ti will say 25.0 degrees C, OK? I'm adding that. And then it says Tf, gives us the temperature final, is 33.9 degrees C, gives us the specific heat of the solution, 4.18 joules per gram degree C. And it gives us these concentrations. That's just to throw us off. But it does give us the volume. So it says 25.0 mils is added to 50.0 mils, OK? So remember I said the volumes are additive. That means that when they add together, they equal the amount that they add, right? So they don't always do that when you're making solutions. So the volume here is going to be, what was it? 25.0 mils plus 50.0 mils, they equal 75. And it also gives us the density of the solution. So the density of the solution is 1.0 grams per mil. So I think that's all the stuff we need. We also need to remember, you guys remember the specific heat equation? Equals delta T, right? So we've got, well, delta T, essentially here. We've got C. But I thought we were looking for delta H of the reaction. That's not pictured here, is it? It's Q, right, remember? So in fact, in this case, Q is delta H of the reaction. So I wanted to point that out to you. OK, so let's, so that's what we're looking for. But do we have the mass of this solution? Can we figure it out? We can figure it out. How? Because we've got what numbers? The volume and the density, right? So let's figure out the mass. So the mass is going to be 75.0 mils. So we've got the mass. And remember, delta T is Tf minus Ti. So 33.9 degrees C minus 25.0. So that's what? 8.9 degrees C, right? OK, so we've got the change in temperature. We've got the mass. And we've got the specific heat, right? Should we be able to find the heat of the reaction? Yes? So let's just plug it in. So let's do this together. So I'm going to put it over here, so we've got some room. So we've got 4.18 joules per 1 gram degree C. We've got the mass, which is 75.0 grams. And we've got the change in temperature, which is 8.9 degrees C. But didn't that tell us we wanted to do kilojoules, right? If we multiply this out, what's it going to give it to us? Joules, right? So why don't we convert right now, OK? So 1,000 joules per 1 kilojoule, OK? So that should give us kilojoules, right? So let's cancel with kilojoules. So 8.9 times 75 times 4.18 divided by 1,000, OK? And how many sick things are we going to do? So the delta H of this reaction is going to be plus 2.8. But are you OK with that? Is it the same answer as me? Oh, hold on. If not, then one of us did something wrong. OK, any questions on this one? Pardon? Oh, yeah. So we want to talk about that. So yeah, so what's happening here? Is this energy or losing energy? Gaining, right? So gaining.