1. The problem statement, all variables and given/known data What is the emf of the galvanic cell Al(s)[Al+3(aq .18mol/liter)  Fe+2(aq .85mol/liter)[Fe(s) 2. Relevant equations 3. The attempt at a solution Al(s) ---> Al+3 + 3e E=-1.676 V Fe+2 + 2e ---> Fe(s) E=-.440V How do we proceed after this, and usually in the textbook questions, the number of electrons that are in each reaction are the same, so in this how do we correct that? Do we multiply everything on the top reaction with 2, including the "E", and the bottom reaction with 3, again including the E? And do we switch the signs for these, or do we just take them as it is?