Why is the rusting of iron accelerated by NaCl?
821724
Rusting of iron is an oxidation/reduction process which means there is a transfer of electrons.  Any soluble ionic compound will facilitate the transfer of the electrons and accelerate the oxidation process.
462127
Chromium has been added, so it is less likely to rust (thus "stainless")
1420
Good question.   Could be a number of reason, but my guess would be that you have some salt in your boiling water.    When NaCl solution is placed in a flame the Na cation gets ionized and yellow light is given off.    It doesn't take much salt for you to see this effect.   You will see this even with regular tap water, since it also has a small amount of salts dissolved in it.    \nIn fact, standard distilled water is usually not pure enough to avoid this effect.    That's why chemist buy special stills to make ultrapure water for experiments.
156880
if iron comes into contact with moisture and air, it starts to rust.The surface of iron is painted because it prevents iron from coming into contact with air and moisture.
730355
Why not? Iron and oxgen form a number of compounds of both determinate and indeterminate composition. Someone want to give me the exact formula for rust?
865835
A few types of corrosion are:\n1) PITTING: Pitting corrosion is quite often evident on metal surfaces where no uniform corrosion is present and is usually highly localized. Pitting usually proceeds fairly rapidly and is accelerated by the presence of chlorides and is particularly common at the base of breaks in coatings. Pitting corrosion takes advantage of the different metallurgical phases present on the surface of most common modern alloys. Generally it is considered to be the product of localized anodic dissolution where the anodic portion of the corrosion cell is dwarfed by the larger cathodic portion.\n\n2)STRESS CORROSION CRACKING : Stress corrosion is the product of tensile stress (including residual stress remaining after fabrication) and localized corrosion which combine to produce a brittle cracking of metal under certain conditions. Examples of environments which enhance stress corrosion are high pH amine solutions for most common steels and chloride bearing solutions for most stainless steels as well as certain aluminum alloys.\n\n3) CREVICE CORROSION: Crevice corrosion occurs in sheltered, localized areas such as  crevices, joints, bolted and threaded parts and under existing corrosion deposits. It is the result of concentration of salts, acids and moisture which results in the formation of an occluded corrosion cell in such sheltered areas. A small anode is created in the crevice with the remainder of the body acting as a large cathode so corrosion at the crevice is highly accelerated as well as concentrated.\n\n4)HIGH TEMPERATURE: Under very high temperature metals need only the presence of oxygen or other oxidizing gases to corrode. This type of corrosion is referred to as high temperature oxidation, scaling or tarnishing and requires neither moisture nor dissolved electrolytes (salts, acids) to proceed.
831735
Reaction between the battery and traces of iron in the concrete. Electrolyte level may have been low already.
550877
Well my man fatigue limit cannot tend to infinity... you joking??????? anyways non ferrous metals have higher fatigue limit coz no other metal corrodes as fast as iron.... got it?
1165664
As  far as I know, galvanizing involves coating metals like iron with zinc. If you understand redox, then zinc is a stronger oxidizing agent than iron i.e. it will react before iron gets a chance to become rust. When zinc reacts with water, it makes zinc hydroxide which coats the outer layer of the galvanized metal. Zinc hydroxide, unlike rust, doesn't look too bad and prevents any further reaction from occuring.
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.
408591
When iron turns to rust, the resulting rust is heavier than the original object.
599313
Refer to the electrohemical series (see source).  The answer depends on whether the conditions are such that iron is oxidized to Fe2+ or Fe3+.  In the case of iron metal being oxidized to Fe2+, the correct order is:\n\nMg, Zn, Fe, Sn, Pb
146495
if metal rusts, the iron is being oxidized so it is a chemical change.
972949
WARNING:  Answer is NOT OXYGEN.\n\nIt is true that when metals rust, it forms metal oxides.  But by definition, Catalyst Speeds up the process of the Rxn but does not get used up.  However as you can see in the equation below, Oxygen is consumed with metal to for metal oxide.  Therefore Oxygen CAN'T be a catalyst.  It is a reactant.\n\nFe + O2 ---> Fe2O3\n\nThe Correct answer is SALT.  (Sodium in NaCl for an example)\n  \nRust is the process of metal oxidizing into metal oxide.  The oxidation needs a transfer medium to occur, such as water. Salt in the water speeds up the oxidation process by acting as a catalyst.  The salt is never used up and the problem with salt is that even when water is gone, it remains and wait to restart the forming of rust once more moisture is present.  This is why metals rust much easily in salty areas such as beaches and cold states where they use salt to melt the icy roads.   \n\nI hope you get my answer in time, if this question if for school.  I know I'm against 3 answers here but let my past records of best answers speak for itself.
901405
nothing, the salt water will NOT react with iron, however the rion will just replace a few of the ions of the mineral and still probally nothing will happen
32437
What's with this question?  It's becoming a new chicken-or-egg, why-is-the-sky-blue question.\n\nMagnesium acts as a sacrificial anode.\n\nOxygen in the atmosphere reacts with iron to oxidize it in what is called a redox reaction (oxidation/reduction). The redox reaction is defined by the exchange of electrons--uncharged iron will lose two electrons to an oxygen molecule, creating iron oxide. Water quicken rusting by serving as a catalyst. Dissolved oxygen in the water reacts, and as the water dries, the oxygen becomes increasingly concentrated.\n\nEngineers will prevent wide-spread rusting by creating what is called a "sacrificial anode." You might know the names anode and cathode from the ends of a battery. Batteries function by employing two seperate redox reactions, where one end corrodes to release electrons, which travel to the other end and react with metal cations in solution, turning them to a solid metal. The corrosion of iron is prevented by creating a sacrificial anode out of something even more reactive than the iron (usually magnesium). The corrosion of the magnesium releases excess electrons in the iron, which delays corrosion of the iron--oxygen can grab the free electrons created by the corrosion of magnesium without needing to corrode the iron.
137048
it causes them to rust or melt overtime.