3. An underground copper pipe is used to transport oil under a factory. It is very important that this pipe does not oxidize, so engineers use impressed current cathodic protection. a. Would zinc be an appropriate metal to use for cathodic protection? Why or why not? (4 points) b. Engineers attach a sacrificial anode to the copper pipe. To use impressed current cathodic protection, they must attach a battery between the cathode and anode. Which material should the positive side of the battery be attached to? Explain how you know. (4 points)

a) Copper corrosion is prevented by an external current source that provides a condition around the copper that halts the rust through current cathodic protection

Due to the location of the pipeline, an material such as graphite, titanium, or niobium can be used which lasts longer that zinc can be used for longevity of the protection

b) The positive side of the output DC terminals are attached to the anodes such as graphite, while the negative terminals are connected to the copper pipe to be protected

Explanation:

Making the protected metal the cathode will make the metal be the source of electrons into the reaction taking place such that the release of the positive metal ions that results in disintegration takes place at the anode and as such the protected metal made the cathode, to which the negative terminal of the battery is attached is protected.

answer:

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answer:

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explanation: