Calculate the standard cell potential and the standard free-energy change (in kilojoules) for the reaction below. (See Appendix D for standard reduction potentials.) <QUESTION REFERENCES APPENDIX D>

Video transcript

Welcome back everyone. Another video for the reaction below determine the standard cell potential and the standard gives free energy in killer tools. Now, we are given a reaction mos of titanium solid react with three moles of Germanium two plus to produce two moles of titanium, three plus and three moles of Germanium solid. What we're going to do is just look at the reduction potentials. We're given a reduction of titanium three plus into titanium. If we balance this reaction, we're just adding three electrons and producing a neutral titanium. Now, the reduction potential is negative one point 37 balls. For the second half equation, we have Germanium two plus producing Germanium. If we balance it out, we just need to add two electrons. And we're given the reduction potential which is 0.24 volts. If we look at the overall reaction, we notice that we need to flip the first half equation. Now, what do we get if we flip it? Well, essentially we are going to reverse it and we're going to get titanium producing titanium three plus and three electrons. Let's recall that whenever we flip a half equation, we also have to flip the sign of the reduction potential. So we're making it positive 1.37 volts for the second half equation, we're going to leave it as it is because Germanium has a positive charge positive T charge under. So we're going to not modify it. Germanium two plus combines with two electrons to produce neutral germanium. And this gives us the reduction potential of 0.24 volts. Now that we have everything on the correct sides of the hop equations, right? We have neutral titanium, we have Germanium two plus cion. On the reactant side, we can just add up our reduction potentials. And we're going to get the standard cell potential. If we add 1.37 volts and 0.24 volts, we're going to get 1.61 volts. That's our first answer, right. We have obtained the standard cell potential. Now, we also want to calculate the change in the gibbs free energy. Let's recall that delta G knot is equal to negative NFE. Now, we already have our standard cell potential. We will need the five days constant. And eventually, we just want to get the number of electrons transferred. Well, essentially, if we want to balance this equation, there are two ways to do that. Either we find the lowest common multiple between two and three, which is six or we can simply observe the balanced equation according to the balanced equation. We will need two titanium, which gives us six electrons half equation we will need we germanium cations. This gives us six electrons and three germanium solid Adams. Right? So notice that we have six electrons transferred total. This doesn't have an effect on the standard reduction potential. It's only important for the gibbs free energy change. So what we're going to do is take the negative sign from the equation. We're going to take six moles of electrons. That's what we have based on the lowest common multiple. We need to multiply that by the far days, constant 96485 cool arms per mole of electrons. And now we're going to multiply by the potential which is 1.61 volts, we simply want to calculate the result. So what we're going to do is just multiply all of our quantities we're going to take negative six, multiplied by 96,485. And then we are going to multiply by 1.61 volts. So let's go ahead and do that. When we multiply all of these numbers, we get negative 932,000. But in kilojoules, that would be negative 932 kilojoules, right? So essentially we have our answers. The standard cell potential is 1.61 volts and the change in the gibbs free energy would be negative 32 kg joules. Thank you for watching.