What is one effect of galvanic corrosion?

Galvanic corrosion occurs specifically when two dissimilar metals are in electrical contact with each other and are immersed in an electrolyte, such as water. In this scenario, the more anodic (or less noble) metal will corrode faster than it normally would when in isolation, while the more cathodic (or more noble) metal is protected from corrosion. This effect is due to the established electrochemical cell that forms between the two metals, initiating an oxidation-reduction reaction.

Understanding this process is crucial for preventing galvanic corrosion in various applications, such as in piping systems or in structures where different metals might be used together. The presence of an electrolyte is essential for galvanic corrosion to occur, as it facilitates the flow of ions between the two metals. This highlights the importance of considering both the metal types and the environmental conditions to mitigate corrosion risks effectively.

In contrast, the other options do not accurately describe the phenomenon of galvanic corrosion or its effects. For example, galvanic corrosion does not strengthen the weaker metal, nor is it limited to dry environments—it can happen in wet or humid conditions where electrolytes are present. Additionally, while applying a protective coating can help reduce corrosion overall, it does not completely eliminate galvanic corrosion if dis