 Okay, let's try this Arrhenius equation problem. This problem says the variation in the rate constant at two different temperatures for the decomposition of hydrogen iodide gas to hydrogen gas and iodide gases, but give them below. Calculate the activation energy. So, they gave you the data. Let's write down the reactions. So, they were nice enough to give us the data in table form and also to give us the temperature in kelp. That really helps because when you're doing these Arrhenius equations you're going to have to convert your temperatures to Kelvin if they're given to you in Celsius or God forbid Fahrenheit. Okay, so you're going to have to convert it to Kelvin at the end. So, whenever you see a change in temperature and a change in K here, that's clues you into being Arrhenius problem. Okay, and it's asking you to calculate the activation energy too. So, the only way you guys know how to do that is to use the Arrhenius equation. Okay, so at this point. So, let's go ahead and write out the Arrhenius equation. So, ln K2 over K1 equals the negative EA. So, that's the activation energy. So, that's what you're looking for. Or, that's the gas constant, but that's the 8.314. So, that'll be given to you. I'll write it down for you in a second. So, 1 divided by T2 minus 1 divided by T. So, what I'd like you guys to do, so I always like to isolate the variable first thing. So, why don't you guys try to manipulate that equation to isolate the variable. We're solving for EA. So, let's do minus 1 over T. And you, of course, could do this problem without rearranging the equation. You just like plugging things in and then rearranging. That would also work. This is nice because it cancels out all your units right away. So, let's plug all these things into here. And I think we're all in the right units. The Ks, of course, have to be in the same units, which they all know. So, R is, like I said, it's going to be given to you, 8.314 joules per mole. Remember, get familiar with that number so you know when to use it. So, you don't have to memorize it or memorize the number or whatever. You know, just know when you're going to use it. So, let's do this. We got to call one of them K1 and the other one K2 or reaction 1, reaction 2. So, we'll say this one's 1, 2. So, reaction 1, reaction 2. So, this kind of an expanded arm. Joules 1 mole. Okay. So, remember, activation energy, that's an energy value. So, you're going to want it in energy units. So, probably joules is what you want to cancel everything out to. So, let's just make sure. Or, in this case, it's going to be joules per mole, which is a fine energy unit. Notice, like I said, the Ks have to be in the same units and most of the time they are. So, Kelvin divided by, or 1 over Kelvin divided by 1 over Kelvin is going to cancel those Kelvins out. And, like I said, joules per mole is a good energy unit. So, does anybody have any problems up to this point? So, let's go ahead and just plug and check. In whichever order you like to do it in. And, when you get these to be in joules, because joules is a small energy unit. Okay. So, I'm going to erase this part. Can I erase this part? Is it okay with me erasing that? Yes. Okay. So, 1, 4, 2, 0. I assume that's enough. Save things. Let's go back and check. Okay. So, 1, 3, save things. So, that's too many. So, going to be 1.85 times 10 to the 1, 2, 3, 4, 5, 5 joules per mole. Okay. And, if you wanted to put it into kilojoules, you could divide the thing by 1,000 and get the number of kilojoules. Okay. Oftentimes, energy units are written in kilojoules. But, I don't think this one asks this. What to do? Are there any questions on this one?