- Electrochemistry questions
- Redox reaction from dissolving zinc in copper sulfate
- Introduction to galvanic/voltaic cells
- Electrodes and voltage of Galvanic cell
- Shorthand notation for galvanic/voltaic cells
- Free energy and cell potential
- Standard reduction potentials
- Voltage as an intensive property
- Using reduction potentials
- Spontaneity and redox reactions
- Standard cell potential and the equilibrium constant
- Calculating the equilibrium constant from the standard cell potential edited
- Nernst equation
- Using the Nernst equation
- Concentration cell
- Introduction to electrolysis
- Quantitative electrolysis
- Electrolysis of molten sodium chloride edited
- Lead storage battery
- Nickel-cadmium battery
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- Wait why did you assume 25 Degrees Celsius at4:14min? Isn't the point of this equation to determine E at non-STP values?(4 votes)
- Took a while for anybody to respond but I hope this kinda makes sense and is not coming too late.
You would naturally assume 25 degrees celsius (standard temperature) to find the value of E if you start talking about standard cell potential E-zero.(4 votes)
- At3:00to4:32, how can you incorporate this into a MCAT math method? Would like to see the trick for this since there is no calculator. Thanks!(2 votes)
- [Voiceover] We've already seen that the change in free energy, delta G, can be related to the cell potential E by this equation. Under standard state conditions, this would be the standard change in free energy, so delta G zero, which is related to the standard cell potential E zero, all right, by the same equation. This equation down here comes from thermodynamics and we're going to plug in for delta G and delta G zero, so we're going to plug this in for delta G and we're going to plug this in for delta G zero, so that gives us negative nFe is equal to negative nFE zero plus RT natural log of Q, where Q is the reaction quotient. Let's divide everything by negative nF, so we're going to divide everything in here by negative nF, and let's see what cancels out, so all of this would cancel out, all of that would cancel out, and we get the Nernst equation, so let me go ahead and write it. The cell potential, E, is equal to the standard cell potential, E zero, minus RT over nF times the natural log of Q, where Q is the reaction quotient, so this is the Nernst equation. All right, we'll talk about why the Nernst equation is so important, we'll talk more about that at the end of the video. Right now, let's go ahead and derive another form of the Nernst equation. I should say the form when you're talking about a certain temperature, so at 25 degrees C. Most of our reactions take place at 25 degrees C. Well, temperature, temperature in here, this is the temperature in kelvin, so we need to convert to kelvin, so if you add 273.15, you get your temperature in kelvin, so that would be 298.15, so what we're going to do is solve for RT over F to write a different form of the Nernst equation, and so the temperature is 298.15 kelvin, so let's write that in, so 298.15 kelvin. R is the gas constant, so remember the gas constant is 8.314, 8.314 joules over mole kelvin, and F is Faraday's constant. Remember, Faraday's constant from an earlier video. That's 96,500 coulombs per mole, so Faraday's constant is the charge of one mole of electrons. So let's solve for what all this is equal to, This is equal to, this is equal to .0257, and for units, kelvin would cancel out, moles would cancel out, that gives us joules over coulombs which is equal to volts, so this is equal to volts, and we can write another form of the Nernst equation. So, if your reaction's at 25 degrees C, you can write the Nernst equation this way. You could say that the cell potential, E, is equal to the standard cell potential E zero, minus, so all that RT over F is equal to this, .0257, right? So, .0257 volts. We still have n. Remember n is the number of moles, let me use green for that. N is the number of moles of electrons that are transferred in your redox reaction, so we're going to put n in here, and we still have the natural log of Q, the reaction quotient. So here is another form of the Nernst equation. So at 25 degrees, you can use this form, and then we can also write this into base 10, into base 10 logarithm instead of natural log, so we can do that conversion. So we also did that in an earlier video but if you're trying to convert this .0257 you need to multiply by the natural log of 10. This is equal to .0592 so we can write the Nernst equation once again. So, E or the cell potential is equal to the standard cell potential, E zero minus .0592 over n, and we essentially just changed this from natural logarithm to base 10 logarithm so this would be log of Q, log of the reaction quotient. So, here is just another form of the Nernst equation, so why is the Nernst equation important? Why is it useful? It's useful beause it allows us to calculate a cell potential under non-standard state conditions, so think about this cell potential as being the instantaneous cell potential, and you can relate that to the progress of the reaction, right? So as you change concentrations, the reaction quotient Q changes, and that means that the instantaneous cell potential changes, so if you change the concentrations, if you change the concentrations, you're changing the cell potential, and so we'll see more about that in the next video, so I think that the Nernst equation makes much more sense when you do some problems with it, and then you can understand better what it means.