Using reduction potentials

- [Voiceover] Let's say that we're given this reaction and we're asked to find the standard cell potential. We can do that by using our standard reduction potentials. So if we look at this first half-reaction, we see that silver ion, if you add an electron to a silver ion you get solid silver. So gain of electrons is reduction. So this is a reduction half-reaction. If we look at the reaction on the right, we can see that we are reducing silver ions. So here's silver ion which is being reduced to solid silver. So we need this half-reaction as it's written. So this is going to be our reduction half-reaction. So we have Ag plus, so we have Ag plus plus an electron giving us a solid silver here. The standard reduction potential for this half-reaction is positive .8 volts. So this is positive .8 volts. Next, let's look at what else is happening. We're turning solid zinc into zinc two plus ions. How do you turn solid zinc into zinc two plus? Solid zinc would need to lose two electrons to turn into zinc two plus. Loss of electrons is oxidation. So if we go over here to this half-reaction, we can see that this half-reaction is written as a reduction half-reaction. Zinc two plus is being reduced, is gaining two electrons, to turn into solid zinc. We need to write this as an oxidation half-reaction. So it's given to us as a reduction, we need to write it as an oxidation half-reaction, we simply need to reverse it. So we need to start with solid zinc. So we start with solid zinc here. And for solid zinc to turn into zinc two plus ions, we need to lose two electrons. So loss of electrons is oxidation. So we need to find the standard oxidation potential next. And we can do that by looking at our table once again. The standard reduction potential for this half-reaction as it's written is negative .76 volts. Since we reversed this half-reaction, we reversed this half-reaction, we need to change the sign from negative to positive. So for the reduction potential it's negative .76, for the oxidation potential, it's positive .76. So the standard oxidation potential for this half-reaction is positive .76 volts. Next, we need to look at moles. So if we look at our reaction, we have two moles of silver ions being reduced to two moles of solid silver. Down here we have one mole of silver ions being reduced to one mole of solid silver. So we need to multiply everything by two here, so we get two moles of silver ions, which require two moles of electrons, to turn into two moles of solid silver. Now it might be really tempting to say, oh, well then don't we just multiply our reduction potential by two as well? And we don't, for the reason that we talked about in the previous video. Voltage is an intensive property. So it doesn't matter if you're forming one mole of silver or two moles of silver, the voltage is the same. So we're gonna leave the voltage at .8 volts. Alright, next we have the number of electrons equal, so we can add our two half-reactions together to get our overall reaction. So if you add the reduction half-reaction and the oxidation half-reaction, together we get our overall reaction. So the electrons lost by zinc, these two electrons here, are the same electrons that are gained by the silver ions. So those cancel out. And on the left side we would have two Ag plus plus solid zinc. So let's write that in here. Two Ag plus, plus solid zinc, and for our products, so over here on the right, we have two Ag plus zinc two plus. So we have two Ag plus zinc two plus. Notice this is our reaction. So if I box this here, this overall reaction that we've just found, is the same as what we were given in our problem. So we found our overall reaction. But remember, they wanted us to find the standard cell potential. So how do we find the standard cell potential? We talked about how to do this in an earlier video. To find the standard cell potential, you can think about how we found the overall reaction. We added the reduction half-reaction and the oxidation half-reaction together to get the overall reaction. So to find the standard cell potential we need to add the standard reduction potential and the standard oxidation potential together. If we add the standard reduction potential and the standard oxidation potential together we should get the standard potential for the cell. So let's go ahead and do that. The standard cell potential is equal to, this would be positive .8 volts. So positive .8 volts plus positive .76 volts. Plus positive .76 volts. Which is equal to positive 1.56 volts. So the standard cell potential is positive 1.56 volts. Remember, a positive value for your potential means a spontaneous reaction. So this is how to use your reduction potentials to figure out a standard cell potential.