The chart can be used to determine the likelihood of a galvanic reaction, and galvanic corrosion or bimetallic corrosion, between two different metals in a seawater environment. The closer a metal or an alloy is in the galvanic series, the less are the effects of galvanic corrosion compared to those metals far apart. Zn, Ag/AgCl and Cu/CuSO4 reference electrodes Galvanic series chart Galvanic series diagram determines the nobility of metals and semi-metals vs. Top listed metals/alloys are the least active (most noble) and proceeds down to the most active (anodic) metal/alloy. The below diagram lists metals and alloys potential in the order of reactivity in sea water vs. Read more about the electrochemical cell and process of corrosion. The rate of corrosion on the less noble metal is determined by the electrolyte, the difference in nobility and the relative areas of the anode and cathode exposed to the electrolyte. Galvanic cellĪ galvanic cell arise when two metals with dissimilar compositions come into contact in the presence of an electrolyte. The less noble metals becomes the anode and corrodes faster than it would all by itself, while the other becomes the cathode and corrodes slower than it would alone. When two metals are submerged in an electrolyte, while also electrically connected by a metallic conductor, the less noble will experience galvanic corrosion. The more negative a metal or alloy is, the more likely it is to suffer galvanic corrosion. Each alloy or metal has a distinctive corrosion potential.
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