What are the values of x and y for the following reaction if E° =...

Question

What are the values of x and y for the following reaction if E° = 0.91 V and ∆G° = -527 kJ?

Accepted Answer

Hello in this problem. We are asked to or false for the fond reaction. The value of X and Y are three and four respectfully. Were given the change in Gibbs free energy and the standard cell potential. We can relate the change in Gibbs free energy to the standard cell potential and then solve for the moles of electrons, move everything else to the other side. So then we have the change in our it's for energy And a fair day is a charge on one mole of electrons which is 96,485 columns. And we have then our standard cell potential call that volt is equal to a jewel per um and then we're gonna convert our jewels kill jules, You see then the kill jules cancel jules cancels columns, cancels and we're left with moles of electrons. This works out to the 12 moles of electrons. Making use of the charges were provided. We would have C2, the three plus being reduced to form C. We would have D than being oxidized to form D four plus. Then in order for us to be able to combine these two reactions, the modes of electrons being gained will have to be equal to those that are lost. That would tell us then that this first reaction should be multiplied by four and the second multiplied by three. If we do this, then our number of moles of electrons being lost in game will be the same. But we won't have the coefficients that were provided to us in the balanced equation. And so therefore then the charges on X and Y cannot be three and four. So this therefore is false. This corresponds to answer B. Thanks for watching. Hope This help.

What are the values of x and y for the following reaction if E° = 0.91 V and ∆G° = -527 kJ?

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