1. The problem statement, all variables and given/known data Use the Nernst equation and data from Appendix D in the textbook to calculate E cell for each of the following cells. Mg(s)|Mg+2 (0.012 M) || [Al(OH)4]- (0.25M), OH- (0.048M)|Al(s) 2. Relevant equations Ecell = Ecell(standard) - 0.0591/n * log Q 3. The attempt at a solution Half reaction of Mg: -2.356 Half reaction of [Al(OH)4]-: -2.310 Ecell (standard) = -2.310-(-2.356) = .046 V Equation written out in spontaneous form would be... 3Mg + 2[Al(OH)4]- -> 3Mg+2 + 8OH- + 2Al Then solving for Q... which is [product]/[reactant] would be... Q = ([.048]^8 * [.012]^3)/[.25]^2 = 7.79E-16 Number of moles of electrons transferred is 2. Plug everything in... Ecell = .046 - (.0591/2)*log (7.79E-16) Which gives me Ecell = 0.492 V However, the program I'm entering this into says it's incorrect. Any pointers on where I went wrong? Thanks in advance.