Yes, copper makes iron rust faster.
Here's why:
The accelerated rusting of iron in the presence of copper is due to a process called galvanic corrosion, which is an electrochemical reaction.
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Electrochemical Reaction: Rusting is an electrochemical process where iron loses electrons (oxidation) and oxygen gains electrons (reduction). This process creates iron oxide, which we see as rust.
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Galvanic Corrosion: When two different metals, like iron and copper, are in electrical contact in the presence of an electrolyte (such as water, especially saltwater), a galvanic cell is formed.
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Copper's Role: Copper is more noble (less reactive) than iron. This means that iron will preferentially corrode when in contact with copper. Iron acts as the anode (where oxidation occurs), and copper acts as the cathode (where reduction occurs). The electrons released from the iron flow to the copper, accelerating the oxidation of the iron and thus, speeding up the rusting process.
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Electrolyte: The presence of an electrolyte, like water or saltwater, facilitates the flow of ions and completes the circuit, which is crucial for galvanic corrosion.
In Summary:
When copper is in contact with iron in the presence of an electrolyte, it creates a galvanic cell that accelerates the corrosion of iron (rusting). The iron corrodes more quickly than it would on its own because the copper acts as a cathode, drawing electrons from the iron anode.
