Sapling #12 (Week 7/8)

[Jessica Luong 3K]

Calculate the standard free-energy change for the reaction at 25 ∘C. Refer to the list of standard reduction potentials.

2Au3+(aq)+3Cr(s)↽−−⇀2Au(s)+3Cr2+(aq)

For this question, I know that I should use deltaG = -nFE. Before that, I should calculate E by using the standard reduction potentials chart. Do I need to multiply these potential values in order to balance the equation or do I keep it as it is?

[Jonathan Haimowitz 3B]

E^∘ is an intensive quantity, so it should not be multiplied.

[Valerie Doan 3I]

You do not need to multiply the . You can only "reverse" it or take the negative, if the reaction is an oxidation half reaction. Note this is not the same as where we were able to multiply it by the same factor that we used for our reaction.