{"id":2638,"date":"2023-10-29T15:42:54","date_gmt":"2023-10-29T15:42:54","guid":{"rendered":"https:\/\/deltar.novanta9.net\/blog\/galvanic-corrosion-a-comprehensive-guide\/"},"modified":"2023-10-29T15:42:54","modified_gmt":"2023-10-29T15:42:54","slug":"galvanic-corrosion-a-comprehensive-guide","status":"publish","type":"post","link":"https:\/\/deltar.it\/en\/blog\/galvanic-corrosion-a-comprehensive-guide\/","title":{"rendered":"Galvanic corrosion – a comprehensive guide"},"content":{"rendered":"

Galvanic corrosion is a chemical and physical phenomenon that affects metals and their alloys when they come in contact with an electrolyte and are electrically connected to a different metal. This type of corrosion is of particular relevance in materials engineering, metalwork preservation, and many industrial and marine applications. To fully understand galvanic corrosion, it is necessary to explore its mechanisms, causes, consequences, and prevention strategies.<\/p>\n

\"Galvanic
taken from Wikipedia<\/figcaption><\/figure>\n[ez-toc]\n

The Mechanisms<\/h2>\n

Galvanic corrosion occurs when two dissimilar metals, or metal alloys, are placed in electrical contact in the presence of an electrolyte, which can be a conducting liquid such as saline water. The metals involved have different electrochemical potentials. In this galvanic pair, the metal with the most negative potential becomes the anode and oxidizes, giving up electrons, while the metal with the most positive potential acts as the cathode and receives electrons.<\/p>\n

The anode undergoes gradual dissolution, with loss of material, while the cathode generally remains intact or may even be protected from galvanic reaction. The rate at which galvanic corrosion occurs depends on the potential difference between the two metals, the conductivity of the electrolyte, and the resistance of the overall electrical circuit.<\/p>\n

Some Metals Commonly Subjected<\/h2>\n