Question: A voltaic cell is constructed with two silver-silver chloride electrodes, each of which is based on the following half-reaction: AgCl(s) + e- = Ag(s) + Cl-(aq). The two cell compartments have [Cl-]= 1.41×10−2 M and [Cl-]= 2.70 M, respectively. What is the emf of the cell for the concentrations given? My Work: I found the standard emf of the cell to be 0 V and then I tried to use the Nernst equation to find emf, but it came out wrong. I also answered a previous multiple choice question which told me that the compartment with the 1.41×10−2 M Cl(aq) is the cathode (I don't understand why though because I thought the more concentrated one was the cathode...) So then here is what I did: Standard EMF = 0-((8.3145*298)/(1*96485)) * ln ((1.41×10−2 M)/2.7) but the answer I am getting is incorrect. Where did I go wrong?