Description Laboratory 6 Procedure:     Electrochemistry: Galvanic Cells and the Calculations                                                                            of Cell Potential Background: Galvanic cells, also called voltaic cells, or battery cells are type of electrochemical cells that in which spontaneous reaction generates an electric current. Here there is an example of spontaneous red-ox reaction that is used in a galvanic cell: Zn(s)   +  Cu2+(aq)   ?   Zn2+(aq)  +  Cu(s) we can separate above equation in two half-reactions: Zn(s)  ?  Zn2+(aq)  + 2e  and   Cu2+(aq)  + 2e  ? Cu(s) As shown in Figure 1. potential, a voltage difference between two half cells, drives electric current. A Galvanic cell consists of: Two electrodes, made of metal or graphite, placed in two separate containers (half-cells):          -anode: oxidation process occurs there, has higher potential so electrons flow away from it.          -cathode: reduction process occurs there, has lower potential, electrons flow toward it. Salt bridge: made of porous get that connects two half cells, only counter ions can flow through it from one solution to another. Figure 1: Zinc-copper galvanic cell. Instead of drawing the diagram, we use the following electrochemical cell notation to describe zinc-copper galvanic cell: Figure 2. Electrochemical cell notation for zinc-copper galvanic cell. Each half-cell has its own potential. The standard potential of the cell Eocell is the resulting potential from combining the potential of each half-cell. Calculation of the standard cell potential can be conducted using either of two methods described below. First method requires combining half-reaction and their standard electrode potential values, reduction and oxidation