Electrons in charge

Question

You perform an electrochemical reaction in which 0.300 mol of Cu+ are reduced to solid Cu

How many coulombs of charge are transferred?

I calculate the columbs correctly 2.84x 10^4 C

But how would I solve for the number of electrons in this amount of charge??

Answer 1

Cu⁺ + e- ==> Cu(s)

moles of electrons transferred = 0.3 mols Cu⁺ x 1 mols e- / mol Cu⁺ = 0.3 mols electrons transferred

0.3 mols e- x 96485 C / mol e- = 28946 C (2.89x10⁴ C) not sure why you got 2.84x10⁴ but not significant

The number of electrons can be calculated without using the coulombs at all. Since 0.3 mols of electrons are being transferred, you can simply use Avogadro's number...

0.3 mols electrons x 6.02x10²³ electrons / mole = 1.81x10²³ electrons

Am I maybe missing something in this problem? It seems pretty straight forward.

Answer 2

Divide the total charge by the charge per electron (1.6 x 10^-19 Coul/election.)