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How does a sacrificial anode protect a metal from corrosion? - Leaving Cert Chemistry - Question B - 2005

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How does a sacrificial anode protect a metal from corrosion?

Worked Solution & Example Answer:How does a sacrificial anode protect a metal from corrosion? - Leaving Cert Chemistry - Question B - 2005

Step 1

Sacrificial anodes oxidize more easily

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Answer

A sacrificial anode is a metal that is more reactive compared to the metal it aims to protect. When placed in an electrolytic environment, the sacrificial anode will oxidize preferentially, losing electrons and forming positive ions. This process effectively removes the tendency for the protected metal to corrode.

Step 2

Higher in the electrochemical series

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The sacrificial anode is higher in the electrochemical series than the protected metal. This positioning means it is more likely to undergo oxidation, leading to its own corrosion while safeguarding the less reactive metal.

Step 3

Formation of an electrolytic cell

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Answer

In doing so, the sacrificial anode forms an electrolytic cell where the protected metal serves as the cathode. Since the cathode gains electrons, this further reduces the likelihood of corrosion on the protected metal.

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