electrochemistry principle in the preventatin of rusting?
150659
You may be referring to a sacrificial anode?\n\nSometimes, in order to prevent something from rusting (like a metal water pipe or the hull of a ship), you sacrifice a more reactive metal to corrode first.\nFor example, if you wanted to protect an Iron water pipe from rusting, you could electrically conect it to a "sacrifical" piece of Magnesium (a more reactive metal)m this way, the Mg will corrose first, keeping the Iron safe.\n\nEdit:\nYou wouldnt mix the sacrifical metal in with the metal your trying to protect, then you'll just get an object with a bunch of holes in it (where the other metal was eaten away).  You would electrically connect the sacrifical electrode to the other metal with a wire or something of that sort, then as the sacrificial electrode is corroded away, the other metal stays perfectly intact.\nI think in real life Magnesium is a very common metal to use since it is so high up in the reactivity series and not insanely expensive. Silver doesnt corrose very much at all, it wouldnt work as a sacrifical electrode, not would it need one very badly.
53096
Near East, about 100 BC, it is believed from archaeological finds - ceramic vessels with metal rods, thought to have contained saline solutions.\n\nModern use of batteries was introduced by Galvani around 1790.\n\nThe principle is the same as for modern batteries: connected galvanic half-cells. The use seems to have been for electrolytic coating.
433170
The company I work for does Salt Spray Analysis. it's used to find out how well a coating holds up under controlled conditions. Salt water is very corrosive to most metals and is a good medium for testing for corrosion.\n\nBasically, a part that has a coating (paint, Anodize, Nitride, Black Oxide,...) is placed in a sealed tank. The tank sprays water with a particuar amount of salt in it into the chamber. The parts are checked every hour, 2 hours, 6 hours...as directed by the requirements. As soon as ANY rust is found, the testing stops and the amount of time it took for the rust to show is recorded. 300 hours is very good for any type of paint.
909393
B.\n\nthe process is called passivation. and may be increased to a greater extent on purpose by electrolysing aluminum in acid to increase the oxide layer. this is called anodizing.
1161774
because it stops corrosion to the steel which would rust and therefore increases the shelf life of the wire the same as it would mig or gas welding filler\n\ngaz
394719
Rust is a chemical reaction involving iron and oxygen.  Melting metal is simply a physical reaction changing the state of its matter, so melting the metal wouldn't get rid of the rust to the best of my knowledge.  IT might however make it easy for you to seperate the rusted and non rusted parts of the metal, but then again it might make it a total mess lol
139943
corrosion is normally the oxidation of the metal, painting it stops the air getting to the metal and therefore stops the oxidation.
550059
Rust is the substance formed when iron compounds corrode in the presence of oxygen and water. It is a mixture of iron oxides and hydroxides. Rusting is a common term for corrosion, and usually corrosion of steel.\n\nIron is found naturally in the ore haematite as iron oxide, and metallic iron tends to return to a similar state when exposed to air, (hydrogen, oxygen, nitrogen, etc.) and water. This corrosion is due to the oxidation reaction when iron metal returns to an energetically favourable state. Energy is given off when rust forms. The process of rusting can be summarized as three basic stages: The formation of iron(II) ions from the metal; the formation of hydroxide ions; and their reaction together, with the addition of oxygen, to create rust.\n\nIron is the main component of steel and the corrosion of steel is observed more frequently, since iron is rarely used without alloying in the present day.\n\nWhen steel contacts water, an electrochemical process starts. On the surface of the metal, iron is oxidized to iron(II):\n\n    Fe → Fe2+ + 2e−\n\nThe electrons released travel to the edges of the water droplet, where there is plenty of dissolved oxygen. They reduce the oxygen and water to hydroxide ions:\n\n    4e− + O2 + 2H2O → 4OH−\n\nThe hydroxide ions react with the iron(II) ions and more dissolved oxygen to form iron oxide. The hydration is variable, however in its most general form:\n\n    Fe2+ + 2OH− → Fe(OH)2\n    4Fe(OH)2 + O2 → 2(Fe2O3.xH2O) + 2H2O\n\nHence, rust is hydrated iron(III) oxide. Corrosion tends to progress faster in seawater than fresh water due to higher concentration of sodium chloride ions, making the solution more conductive. Rusting is also accelerated in the presence of acids, but inhibited by alkalis. Rust can often be removed through electrolysis, however the base metal object can not be restored through this method.
812124
1) Depends on environmental conditions\n2) Oxidation of iron--- 2Fe + 3O2---> 2Fe2O3\n3) Not easily.  To remove rust, phosphoric acid (naval jelly) is good\n4) Ultimate weapon: Cadmium plate, epoxy primer, epoxy finish coating.
1157885
There are a vast number of water soluble corrosion inhibitors.\n\nAt the simple end of the scale - Sodium nitrite, sodium tolytriazole, zinc phosphate, borates, molybdates, vanadates and chromates all inhibit rust.\n\nThere are also proprietary organic compounds (some phosphate esters, ethanolamides, etc) also inhibit rust.\n\nIt all depends on whether you want the inhibition to be short lived or long lived (nothing is "permanent") and whether the inhibition is an "in use" inhibitor (like, say, a corrosion inhibitor in cooling water) or "static" (like phosphate "rust converters" used prior to painting.
339643
You need a reference table and some instruction. Go to this site and scroll down to electrochemistry. Good luck!\nhttp://spiderpong.sitesled.com/chemistry_12_handouts.htm
1155855
Possibly the material underneath the stainless is corroding and the rust found a way through. It's not necessarily solid stainless steel.
876346
Corrosion is defined as: the chemical or electrochemical reaction between a material (usually a metal) and its environment that produces a deterioration of the material and its properties.\n\nAny chemical (or electrochemical) that will deteriorate one or more properties of the composite will be sufficient.\n\nTake a simple electrochemical reaction, for example - without a UV coating, fiberglass (which happens to be a composite) loses tensile strength on prolonged exposure to sunlight.
882235
In an electrolytic cell you can plate most any metal that doesn't quickly react with the solvent and its solutes.  The force of the copper ions gaining electrons at a negative charged zinc electrode is certainly possible.\n\nSince the copper would receive two electrons and go from a +2 to a zero oxidation state, you would say that it is being reduced.
491586
Metallic corrosion is basically a redox reaction where the metal is oxidised by the oxygen in the air and sometimes assisted by the presence of water.
128014
Not every kind of paint will do.\n\nThe effect is quite simple: if the paint manages to separate the metal from all oxidizing agents (air, water...), there is no chance of an electron transfer between the metal and the corrosive agent, and hence no corrosion.\n\nThere must be no gaps in such a paint or protective layer of plastics.\n\nUsually, this cannot be guaranteed, which is why special coating paints containing metallic zinc or magnesia as sacrificial electrodes are used below the actual paint.
1066233
Unless they're rechargable batteries no.  If they are take into account if and what water they were exposed to.  Salt water corrodes things so if it came into contact with it just dispose of the batteries.  Battery acid is no fun and ruins clothes and burns like hell.  If it's fresh you have less chance of corrosion.