 So, let's do this one, the last one of the day, it says calculate the equilibrium constant Keq at 25 degrees Celsius for the galvanic cell reaction shown on the board, okay? So that's a balanced, a redox reaction and acidic solution, hopefully you guys can tell that. We're going to have to split this reaction up to figure out, well, what's the number of electrons transferred, okay? So how do we do this? Well, first thing I would like to do, because they don't give you too much information in this equation, let's, or this problem, let's figure out what equation are we going to use. So we're going to use the standard cell potential equation. So E cell, like that, equals, so this is for standard conditions, 0.0592 volts divided by N times the log of Keq, okay? So that relates E cell, which we have up here, to Keq, which is actually what we're looking for. Okay? Is everybody okay with that? Yes. Okay, remember this N, right, that's the number of electrons transferred. So, pardon me, how do we figure that out? Well, we're going to have to break this thing up into its half reactions. So like we said, this is a balanced reaction already, so that was nice, and it's in acidic solution. So we can kind of avoid worrying about that part and about that part if you remember how to balance an acidic solution. And in fact, all you really have to do is figure out one of these half reactions, and the other one will be the same amount of electrons transferred, okay? So let's, well, we could do one or both of them. Let's just do one for right now, the more obvious one. F e 5 F e 2 plus a quiz goes to 5 F e 3 plus a quiz, okay? So 5 times 3, that's 15, right? 5 times 2, that's 10. So what do we need? We need 5 electrons here, okay? So plus 5 electrons, so like that. So if you did the other half reaction, you would find that we'd be adding 5 electrons here. We don't have time to do that right now though, okay? So let's just write down our n equals 5 there, okay? So we have our e cell, let's give it to us up here. We have our n now, we just don't have k e q. So let's rearrange this equation to solve for k e q. So e cell, we'll multiply both sides by n, so standard e cell times n, like that, divided by 0.0592 volts equals the log of k e q. So what you do here now is you're recording right now, okay? So k e q, we're going to raise both sides to the 10, okay? So k e q equals 10 to the deletious plug-in check, so 10 times 5, like that, 0.7 4 times 5 divided by 0.0592. So we get up here 62.5, so 10 to the 62.5 is going to be 3.2 times 10 to the 62, and that's your k e q, okay? Any questions on that one? Yeah, okay. Okay, cool. Thanks, everyone. Bye-bye. Thanks, everyone. Bye-bye.