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Two types of electrochemical cells: (1) Voltaic (galvanic)  spontaneous [product-favored] redox rxn to generate electric current; (2) Electrolysis cell  uses electric current to cause a nonspontaneous [reactant-favored] rxn to occurAnode  oxidation occursCathode  reduction occursReduced (Oxidizing Agent) & Oxidized (Reducing Agent)Stuff on upper left side of table is stronger oxidizing agent (reduced) & stuff on lower right side is stronger reducing agent (oxidized)When looking at whether something is being oxidized or reduced look at subscripts not the big numbers. Platinum, gold, and graphite are used as inert electrodes. E˚Cell < 0  reactant-favored E˚Cell > 0  product-favoredFarraday’s Constant = 96,500 C/mol e- 1 Volt (V) = 1 J/C 1 ampere (A) = 1 C/sCorrosion  oxidation of metals that cause the metal to deteriorate ( Fe2O3H2O). The water isa solution of ionic compounds (NaCl). Think of this as a voltaic cell. Water is the anode and iron is the cathode. The solution serves as a salt bridge and the iron itself acts as a conductor.Zinc and Iron (Write what happens):Corrosion control  (1) cover the surface; (2) sacrificial metal. Sacrificial metal (galvanized steel  surface covered with Zn(s))Al2O3  sticks to the Al surface it prevents additional oxygen from getting to Al surface ; you don’t get further erosion (already a thin layer of corrosion on the surface). Oscillating rxn  multiple step rxn (orange dark blueclear) this cycle continues to occur with stir


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