How is steel protected from corrosion?
437017
anti rust paint called red oxide primer , don't forget this
769099
Iron is stronger and steel of course is stronger still.  Further, iron corrodes only if not cared for.  Copper will form a patina over time even if cared for.
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.
123171
You guys are all close.\nGalvanise is a noncorosive protectant put on metals to protect from rust and carosion.\n\nSteel is a composit make up of different metals (one of which is iron) and carbin to acheave it's spacific purpose of malabulity (able to bond or weld) and strength and flexabulity (usually for structures like buildings).\n\nIron is not widley used in pure form because it is brittle.  You will usually only find iron in castings wich are case hardened for toughness like in engine blocks wher flexabulity is a bad thing.
413110
because they are made of steel
1090211
Galvanized metal is a tin and carbon steel alloy. It corrodes at a slower rate of speed.
139943
corrosion is normally the oxidation of the metal, painting it stops the air getting to the metal and therefore stops the oxidation.
513062
Sorry, what is LCC?  Low carbon (?)\n\nThe only way to harden a steel alloy material by air cooling is if the alloy content is quite high - this is the reason for adding the alloys.  If you don't have high alloy content, you MUST quench to harden the steel.\n\nYou're going to need a carbon content above 0.3% to see any improvement in properties from quenching.  \n\nAnother heat treatment cycle on steel is case-hardening - this would improve surface hardness.
348589
As the above answerer states, you don't need to - titanium won't rust; rather it develops a protective, inert oxide layer in air, just like aluminum has it's protective  inert oxide layer - Al2O3.\nIron and steel rust/oxidize in air and it can prevented by giving a coating of zinc, chromium, or magnesium on it.
295425
"The steels used for spring making depend on the application and type of spring. They range from plain carbon grades in the range 0.5% to 1.00% C. to Chromium, Chromium-Vanadium, Nickel-Chromium-Molybdenum, Silico- Manganese and Silicon-Manganese-Chromium-Molybdenum types." (From ref. 1)\nI don't know about the other alloys, but plain carbon steels can be tempered to spring metal, they call it "blue tempering". It's tempered to a trade-off between hardness and brittleness. Techniques of tempering (including blue tempering with reference to watch springs) are discussed in the ref.
686818
stainless steel is rust proof anyway, to do this, zinc is added during the smelting process, this creates a coating over the metal and when it comes into conntact with oxygen and water it forms a clear oxide layer over the metal, hence stopping the steel from rusting
147407
Rusting is a chemical process that, can take place in metals exposed to the atmosphere. Not all metals however rust. Rusting is common with the metal, iron. Certain conditions in the air around a metal have to be present for iron to rust. Iron rust which, generally appears brown, is itself a chemical compound quite different from the iron itself. The rusting of iron can be prevented. In towns and large cities where iron sheets are used for roofing houses, rusting can also take place if the iron sheets are not protected from rusting. \n\nRust is the common name for a very common compound, iron oxide. Iron oxide, the chemical Fe2O3, is common because iron combines very readily with oxygen -- so readily, in fact, that pure iron is only rarely found in nature. Iron (or steel) rusting is an example of corrosion -- an electrochemical process involving an anode (a piece of metal that readily gives up electrons), an electrolyte (a liquid that helps electrons move) and a cathode (a piece of metal that readily accepts electrons). When a piece of metal corrodes, the electrolyte helps provide oxygen to the anode. As oxygen combines with the metal, electrons are liberated. When they flow through the electrolyte to the cathode, the metal of the anode disappears, swept away by the electrical flow or converted into metal cations in a form such as rust.\n\nFor iron to become iron oxide, three things are required: iron, water and oxygen. Here's what happens when the three get together:\n\nWhen a drop of water hits an iron object, two things begin to happen almost immediately. First, the water, a good electrolyte, combines with carbon dioxide in the air to form a weak carbonic acid, an even better electrolyte. As the acid is formed and the iron dissolved, some of the water will begin to break down into its component pieces -- hydrogen and oxygen. The free oxygen and dissolved iron bond into iron oxide, in the process freeing electrons. The electrons liberated from the anode portion of the iron flow to the cathode, which may be a piece of a metal less electrically reactive than iron, or another point on the piece of iron itself.\n\nThe chemical compounds found in liquids like acid rain, seawater and the salt-loaded spray from snow-belt roads make them better electrolytes than pure water, allowing their presence to speed the process of rusting on iron and other forms of corrosion on other metals.
123326
Most corrosion is on the outside so it really doesn't make a difference, hot or cold. What determines corrosion is the \nenvironment outside of the pipe.
118571
corrosion is actually oxidation. A chemical reaction between oxygen and various materials such as metal. Painting metal prevents oxygen from reaching the metal and stops the chemical reaction.
58800
Iron produces rust by chemically reacting with Oxygen from the atomosphere. Oxygen can easily form Ferrous/ or ferric oxide (i.e., oxides of iron) reacting with iron. We call these iron oxides as rust. The coating of tin protects iron from contact of atomospheric oxygen. That is how tin coatings prevent iron from rust.
186001
u forgot to put the foloowings to choose from...\nbut still here are some ideas for u...\nTO PREVENT RUST, KEEP METAL SURFACE DRY - OR ADD A COATING \nRust is corrosion that affects ferrous metals such as iron and steel. In many cases, water vapor must be in the air before rust can occur. With iron, for example, 40 percent humidity must be present before rust will start to occur. The best way to prevent corrosion is to keep metal surfaces dry. Isolating the metal by coating it with paint, lacquer or wax is another good way to prevent corrosion. \n\nBefore coating a metal surface, remove all traces of rust. Then apply a primer and finish with paint. It's best if the paint and primer are the same brand; they usually are formulated to work together. Metals such as brass, copper or aluminum are best protected with either wax or by spraying them with lacquer or clear varnish. \n\nRust also can attack metal in inaccessible areas. Corrosion occurs inside a home hot-water heater, for example, because the ions circulating in the water make it easy for dissolved oxygen to pull the electrons from the interior surface of the metal tank. \n\nRust that occurs in localized areas is called localized corrosion. There are three types: galvanic, crevice and pitting. \n\n- Galvanic corrosion: It occurs whenever two dissimilar metals contact each other. This creates a flow of electrons between the metals that eventually causes them to disintegrate. One way to prevent this corrosion is to replace one metal piece with another that is compatible with the mating piece.\n\nFor example, many aluminum storm doors have steel rivets holding the hinges or closing piston in place. Often, corrosion starts around these fasteners, then works to the adjacent aluminum panels. Drilling the corroded fasteners out and replacing them with aluminum pop-rivets will stop the galvanic corrosion before it spreads.\n\n- Crevice corrosion: It occurs around the joints and seams of metal fixtures where dirt accumulates. By itself the dirt is not particularly harmful, but it allows moisture to collect; this causes corrosion. Joint and seam corrosion is a common occurrence on gutters and downspouts. Clean them often to keep dirt and leaves, which retain moisture, from building up. If rust is present, remove it with a flexible sanding wheel chucked in an electric drill, then prime and paint the bare metal.\n\n- Pitting corrosion: It occurs outdoors when the wind bombards metal surfaces with minute particles of dirt, salt or sand and creates microscopic craters that retain moisture. At first, the corrosion is limited, then quickly escalates into a formidable problem. Outdoor electrical conduits, television antenna masts, metal windows and doors, and children's play equipment are a few of the items that receive constant assault from air-borne particles and are subject to pit corrosion. This type of corrosion is severe near the seashore and is most noticeable on the side of the house that faces the prevailing winds. Check exposed metal surfaces often; sand and paint them if they show signs of pitting.
930912
What you are really asking, is what chemicals in water can corrode Chromium and Vanadium, since that is what makes stainless steels 'stainless'.\n\nBasically, anything that will form free radicals can react with these metals.  Common culprits include Chlorides, Flourides, and the like,  but also such things as (bi)carbonates and nitrates can form weak acids that can attack Cr and Va.