 Okay, so let's attempt this problem. So using the Nertz equation, we're going to calculate the cell potential. So we're testing a opaque cell consisting of a zinc 2 plus half cell and hydrogen. Proton half cell under the following conditions. The zinc 2 plus concentration is 0.010 molar. Proton concentration is 2.5 molar and the pressure of hydrogen is 0.308 AM. So calculate the cell potential at 298.25 kelp. Okay, so remember if you're going to do it at 25 degrees Celsius or that 298 kelp, that's going to be the Nertz equation that's reduced to that 0.0592 volts per hand. So, oh, we're using the Nertz equation. That's a particular problem. So the first thing we want to do, of course, is balance the two half reactions. So if you need to go back to your half reaction list and look at, okay, so we're going to have, in this case, proton. So the two protons plus two electron. You guys remember the potential for that one? Zero, right? That's the reference potential. Okay, so that thing is good to memorize. Okay, that particular 0.00 volts per second. Okay, that's probably the best way to describe it. And then the zinc half reaction is going to be zinc solid that goes to zinc 2 plus aqueous plus two electrons. And then, of course, in this case you're going to have to look at your table and figure out what the potential that is. And I looked at the table and it's 0.76. So now, of course, we should balance these equate two half reactions and hopefully you can see they're already balanced for us. It's kind of convenient. So let's write out the whole reaction. So cancel, cancel, get two protons aqueous plus solid. You shouldn't be able to figure out what the cell potential is, right? So that's going to be, you guys remember, the E, I'll help you out. Keta minus E and so we want this to be positive. Which one's going to be the cathode then? Top or bottom? Top one. Okay, is everybody okay with identifying that stuff? Okay, remember the most negative thing is the antipanolvis. So 0.00 volts minus A minus 0.76 volts. I guess one thing that we should say since we're going to be using the Nernst equation is we're going to want to remember or figure out how many moles of electrons have been transferred. So ant, remember. So what is ant in this particular equation? Yeah. And the other thing we want to do, so why were we given these things? Because we need to find Q for the Nernst equation. So I'm telling you all this. Let's write down the Nernst equation. You guys remember what the Nernst equation is? Yeah. So E what? Cell equals what? Standard potential of the cell. So did we figure that out already? Yes. Okay, cool. So, oh, help him. Minus 0.0592 volts over N. Do we have N? Yes. Cool. Times what? Log of Q. So what do we miss? Q. Q. Can we figure that out from our balanced equation here? Yes. Yeah. So what is Q? Let's write it over here. The actual equation for it. So remember for gases, we use the partial pressure. Okay. So hydrogen, the partial pressure of hydrogen. Like that. Times the concentration. It's upstream 2 plus. Very good. Divided by, well, are we going to put zinc in there? No. So divided by the protons then. What do we do to that? So that's Q. Let's see if I know. It's for Q. So let's not put any of the units in there so we don't put it in. So it could be second, right? So it's just kind of a plug and chug. Okay. So let's put everything in there. Any questions on anything like that? Okay. I think the, well, this is kind of a combination of everything that you've learned. Equilibrium stuff, balancing half reactions, figuring out the self potential. So if you can do this, I think you guys are good.