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What Is Corrosion
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In general terms, corrosion is the deterioration of a material by chemical or electrochemical reaction with its surroundings As boatowners, we are most familiar with galvanic corrosion the deterioration of the anode of a galvanic couple resulting from the ow of ions from the anode to the cathode through an electrolyte Relax! Those are just fancy words to describe a very common phenomenon the chemical reaction that takes place inside a battery Figure 58 shows a carbon-zinc ashlight battery (the inexpensive type that comes with electrical toys) If we were to slice the battery in half, we would see a carbon rod in an electrically conductive paste, all inside a zinc-coated can At A we measure the voltage between the carbon rod and the zinc can as 15 volts At B,
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Fig 58 The Battery a Useful Form of Corrosion
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Performing the experiment in Figure 59 will do wonders for your understanding of corrosion on your boat Gather a plastic container of fresh water, a tablespoon of salt, a multimeter, two test leads with alligator clips, and an assortment of metal items I used a stainless bolt, a small piece of aluminum pie plate, and a shaft zinc
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Fig 59 Measuring Galvanic Voltage and Current
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Meter set to Amps
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Zinc
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Meter set to Volts
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I e-
I eStainless
Zinc Electrolyte Carbon
Zinc
Zn++
Cor r osion Pr otection
Corrosion Protection
Switch the multimeter to volts Using the test leads, connect the negative ( ) lead to the zinc and the positive (+) lead to the stainless bolt and lower both pieces into the water Surprised The meter will indicate a voltage Now switch the meter to milliamps You may or may not read any current, but hold on Dump the tablespoon of salt into the fresh water and stir Depending on the sizes of the electrodes, you will now probably measure a current of about a milliamp owing from the stainless bolt to the zinc What s going on When two dissimilar metals are placed together in an electrolyte (electrically conductive medium), one of the metals will assume a higher potential than the other In 1 we learned that current ows only in a closed circuit Two electrodes, immersed in electrolyte, form an open circuit, and no current ows But when we connect the two electrodes, either with a wire or by letting them touch, we complete the circuit and current ows In this case, the current owing through the meter is from the stainless steel electrode into the zinc electrode (Since electrons carry negative charge, the electron ow is actually in the opposite direction, but never mind) Figure 510 shows what is happening to the zinc on an atomic level Zinc atoms are changing into positively charged zinc ions by giving up two electrons These released electrons are owing from the zinc to the stainless through the meter leads, and the newly formed zinc ions are departing the zinc electrode and migrating into the electrolyte the zinc is corroding Continue the experiment if you wish by substituting other pairs of dissimilar metals As long as the electrode metals are different in composition, they will always generate a potential difference, and current will always ow into the lower-voltage metal The voltage difference will be the same, whether the water is salt or fresh The currents, however, will be much greater in salt water due to its greater conductivity The potential difference between any two dissimilar metals can be predicted by consulting a table of galvanic potentials The table lists the potential differences measured between the metal in question and a reference electrode, typically silver-silver chloride Table 51 reproduces the values listed in Table I of ABYC Standard E-2 for metals and alloys in seawater owing at 8 to 13 feet per second (47 to 77 knots), and at temperatures of 50 F to 80 F
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