Shopping on line can be easy, simple and save you lots of money. It can also take a lot of your time, frustrate you, and result in unwanted purchases. Now the same can be said for regular high street shopping, but with the vast opportunity presented by the Internet it will pay you to spend a few minutes reading this and understanding how to better optimize your Rust shopping experience:
1. Compare - without doubt the biggest advantage that the Rust offers shoppers today is the ability to compare thousands of Rust at a time. This is a great thing, but not necessarily all the time! Too much can be daunting at times so take advantage of the great comparison sites and where possible let them do the hard work for you.
2. Research - if it has been said it will be on the internet. Ignorance is no longer a justifiable reason for buying the wrong thing. Take the time to research in detail everything that you could possible want to know about
3. Testimonials - don't know anybody that has bought a Rust? Wrong! If the Rust is good the internet will let you know. Use the Internet as a friend and get testimonials before you buy.
4. Questions - Got a question about Rust then search the Forums, FAQ's, Blogs etc. Don't be afraid to ask .....
5. Reputation - Never heard of the company selling Rust? Don't worry, no reason why you should know every company in the world, but you know someone that does! Use the internet to find out what people are saying about Rust and build up a picture of their reputation for sales, returns, customer service, delivery etc.
6. Returns - still worried that even after all of the above your Rust wont be what you want? Check out the returns policy. There is so much competition now that someone, somewhere is bound to offer the terms that you are comfortable with.
7. Feedback - happy with your Rust then let people know, after all you are depending on others people input in your buying decision, so why not give a little back.
8. Security - check for the yellow padlock on the Rust site before you buy, and the s after http:/ /i.e. https:// = a secure site
9. Contact - got a question about Rust, or want to leave a comment then check out the sites contact page. Reputable companies have them and respond.
10. Payment - ready to pay for your Rust, then use your credit card or PayPal! Be aware of companies that don't accept them, there may be genuine reasons but given the huge amount of choice you have when buying online there is no reason at all not to buy via credit card or PayPal.
removing rust with sand prior to welding
image:Rust03102006.JPG on the unrusted portions.
Rust is a general term for
iron oxides formed by the reaction of iron with
oxygen. Several forms of rust are distinguishable visually and by
spectroscopy, and form under different circumstances. The chemical composition of rust is typically hydrated
iron(III) oxide (Fe2O3.nH2O), and under wet conditions may include
iron(III) oxide-hydroxide (FeO(OH)).
Rusting is the common term for corrosion of iron and its alloys, such as
steel. Although oxidation of other metals is equivalent, these oxides are not commonly called rust.
As rust has higher volume than the originating mass of iron, its buildup may force apart adjacent parts - a phenomenon known as
rust smacking.
Chemistry
The rusting of iron is one of the more widely used examples of corrosion. This electrochemical process requires the presence of water,
oxygen and an
electrolyte and leads to the formation of hydrated iron
oxides.
Net reactions
The overall outcome of rust formation involves reaction of iron with varying amounts of oxygen and water.
- 2Fe + O2 + 2H2O = 2Fe(OH)2
- 4Fe + O2 + 6H2O = 4Fe(OH)3
- 4Fe + O2 + 2H2O = 2Fe2O3•H2O
- 6Fe + 4O2 = 2Fe3O4
Mechanism
Pure, solid iron oxidizes in water:
Fe(s) => Fe2+(aq) + 2e-These electrons will quickly react with the disassociated hydrogen ions (in H3O+(aq) form) and the dissolved oxygen in the water (O2(aq)):
4e-(aq) + 4H3O+(aq) + O2(aq) -> 6H2O(l)Therefore, as seen from the above equation, the more acidic the water, the greater will be the rate of corrosion (since the concentration of H3O+(aq) will be greater.) At extremely low pH’s, the hydrogen ions will react with the
electrons producing hydrogen gas instead:
2H+(aq) + 2e-(aq) -> H2(g)Thus, as seen from the above equations, the pH of the solution (whether it is pure water or water containing electrolytes) rises. This leads to the formation of OH- ions (in cases where the body of water is significantly large, the
pH does not rise as sharply, but this is of no consequence since OH- ions are always present, even in pure
water.) The cations then react with the OH- or even the H+ ions and dissolved oxygen to form a variety of compounds, which constitute rust:
Fe2+(aq) + 2OH-(aq) -> Fe(OH)2(s)4Fe2+(aq) + 4H+(aq) + O2(aq) -> 4Fe3+(aq) + 2H2O(l)Fe3+(aq) + 3OH-(aq) -> Fe(OH)3(s)From the above equations, it is seen that the pH and amount of dissolved oxygen can affect the outcome of the reactions. In water with limited dissolved oxygen Fe3O4(s) is formed, which is a black solid and commonly called
lodestone:
6Fe2+(aq) + O2(aq) + 12OH-(aq) -> 2Fe3O4(s) + 6H2O(l)The porous Fe(OH)3 rust can slowly disintegrate into a crystallized form, which is the familiar red-brown rust:
2Fe(OH)3(s) -> Fe2O3•H2O(s) + 2H2O(l)Iron oxide (FeO) can also be formed. The presence of other ions, such as
calcium or calcium carbonates reacts with the iron
hydroxides and iron
oxides to form a variety of precipitates.Other
metals corrode via similar chemical processes.
Rust prevention
Hydrated rust is permeable to air and water, allowing the metal to continue to corrode - internally - even after a surface layer of rust has formed. Given sufficient hydration, the iron mass can eventually convert entirely to rust and disintegrate. Corrosion of aluminium is different from steel or iron, in that aluminium oxide formed on the surface of aluminum metal forms a protective, corrosion resistant coating, a process known as passivation.
Stainless steel similarly resists rusting by forming a passivation layer of
chromium(III) oxide. This is also true of
magnesium, copper,
titanium, and
zinc.
Galvanization consists of coating metal with a thin layer of another such metal. Typically, zinc is applied by either
hot-dip galvanizing or electroplating. Zinc is traditionally used because it is cheap, easy to refine and adheres well to steel. In more corrosive environments (such as at sea)
cadmium may be used. Galvanization often fails at seams, holes and joints, where the coating is pierced. In these cases the coating provides
cathodic protection to metal, where it acts as a galvanic anode rusting in preference.
More modern coatings add aluminium to the coating as
zinc-alume, aluminium will migrate to cover scratches and thus provide protection for longer. These rely on the aluminium and zinc oxides protecting the once-scratched surface rather than oxidizing as a sacrificial anode.
There are several other methods available to control corrosion and prevent the formation of rust, colloquially termed
rustproofing.
- Cathodic protection makes the iron a cathode in a battery formed whenever water contacts the iron and also a sacrificial anode made from something with a more negative electrode potential, commonly zinc or magnesium. The electrode itself doesn't react in water, but only provides electrons to prevent the iron rusting.
- Bluing (steel) is a technique that can provide limited resistance to rusting for small steel items, such as firearms; for it to be successful, water-displacing oil must be rubbed onto the blued steel.
- Corrosion control can be done using a coating to isolate the metal from the environment, such as paint. Large structures with enclosed box sections, such as ships and modern automobiles, often have a wax-based product (technically a slushing oil) injected into these sections. This may contain rust inhibiting chemicals as well as forming a barrier. Covering steel with concrete provides protection to steel by the high pH environment at the steel-concrete interface. However, if concrete covered steel does corrode, the rust formed can cause the concrete to spall and fall apart. This creates structural problems.
To prevent rust corrosion on automobiles, they should be kept cleaned and waxed. The underbody should be sprayed to make sure it is free of dirt and debris that could trap moisture. After a car is washed, it is best to let it sit in the sun for a few hours to let it air dry. In winter, or in salty conditions, cars should be washed more regularly as road salt (calcium chloride) can accelerate the rusting process.
References
See also
External links
- A Primer on Rust, thorough rust prevention and removal information
- Rust Removal and Prevention Articles
removing rust with sand prior to weldingimage:Rust03102006.JPG on the unrusted portions.
Rust is a general term for iron oxides formed by the reaction of iron with
oxygen. Several forms of rust are distinguishable visually and by
spectroscopy, and form under different circumstances. The chemical composition of rust is typically hydrated
iron(III) oxide (Fe2O3.nH2O), and under wet conditions may include iron(III) oxide-hydroxide (FeO(OH)).
Rusting is the common term for
corrosion of iron and its alloys, such as steel. Although oxidation of other metals is equivalent, these oxides are not commonly called rust.
As rust has higher volume than the originating mass of iron, its buildup may force apart adjacent parts - a phenomenon known as
rust smacking.
Chemistry
The rusting of iron is one of the more widely used examples of corrosion. This electrochemical process requires the presence of
water,
oxygen and an electrolyte and leads to the formation of hydrated iron oxides.
Net reactions
The overall outcome of rust formation involves reaction of iron with varying amounts of oxygen and water.
- 2Fe + O2 + 2H2O = 2Fe(OH)2
- 4Fe + O2 + 6H2O = 4Fe(OH)3
- 4Fe + O2 + 2H2O = 2Fe2O3•H2O
- 6Fe + 4O2 = 2Fe3O4
Mechanism
Pure, solid iron oxidizes in water:
Fe(s) => Fe2+(aq) + 2e-These electrons will quickly react with the disassociated hydrogen ions (in H3O+(aq) form) and the dissolved oxygen in the water (O2(aq)):
4e-(aq) + 4H3O+(aq) + O2(aq) -> 6H2O(l)Therefore, as seen from the above equation, the more acidic the water, the greater will be the rate of corrosion (since the concentration of H3O+(aq) will be greater.) At extremely low pH’s, the
hydrogen ions will react with the electrons producing hydrogen gas instead:
2H+(aq) + 2e-(aq) -> H2(g)Thus, as seen from the above equations, the pH of the solution (whether it is pure water or water containing electrolytes) rises. This leads to the formation of OH- ions (in cases where the body of water is significantly large, the
pH does not rise as sharply, but this is of no consequence since OH- ions are always present, even in pure water.) The
cations then react with the OH- or even the H+ ions and dissolved oxygen to form a variety of compounds, which constitute rust:
Fe2+(aq) + 2OH-(aq) -> Fe(OH)2(s)4Fe2+(aq) + 4H+(aq) + O2(aq) -> 4Fe3+(aq) + 2H2O(l)Fe3+(aq) + 3OH-(aq) -> Fe(OH)3(s)From the above equations, it is seen that the pH and amount of dissolved oxygen can affect the outcome of the reactions. In water with limited dissolved oxygen Fe3O4(s) is formed, which is a black solid and commonly called lodestone:
6Fe2+(aq) + O2(aq) + 12OH-(aq) -> 2Fe3O4(s) + 6H2O(l)The porous Fe(OH)3 rust can slowly disintegrate into a crystallized form, which is the familiar red-brown rust:
2Fe(OH)3(s) -> Fe2O3•H2O(s) + 2H2O(l)Iron oxide (FeO) can also be formed. The presence of other ions, such as calcium or calcium carbonates reacts with the iron hydroxides and iron
oxides to form a variety of precipitates.Other
metals corrode via similar chemical processes.
Rust prevention
Hydrated rust is permeable to air and water, allowing the metal to continue to corrode - internally - even after a surface layer of rust has formed. Given sufficient hydration, the iron mass can eventually convert entirely to rust and disintegrate. Corrosion of
aluminium is different from steel or
iron, in that
aluminium oxide formed on the surface of aluminum metal forms a protective, corrosion resistant coating, a process known as passivation. Stainless steel similarly resists rusting by forming a passivation layer of chromium(III) oxide. This is also true of
magnesium,
copper, titanium, and zinc.
Galvanization consists of coating metal with a thin layer of another such metal. Typically, zinc is applied by either
hot-dip galvanizing or electroplating. Zinc is traditionally used because it is cheap, easy to refine and adheres well to steel. In more corrosive environments (such as at sea)
cadmium may be used. Galvanization often fails at seams, holes and joints, where the coating is pierced. In these cases the coating provides
cathodic protection to metal, where it acts as a galvanic anode rusting in preference.
More modern coatings add aluminium to the coating as
zinc-alume, aluminium will migrate to cover scratches and thus provide protection for longer. These rely on the aluminium and zinc oxides protecting the once-scratched surface rather than oxidizing as a
sacrificial anode.
There are several other methods available to control corrosion and prevent the formation of rust, colloquially termed rustproofing.
- Cathodic protection makes the iron a cathode in a battery formed whenever water contacts the iron and also a sacrificial anode made from something with a more negative electrode potential, commonly zinc or magnesium. The electrode itself doesn't react in water, but only provides electrons to prevent the iron rusting.
- Bluing (steel) is a technique that can provide limited resistance to rusting for small steel items, such as firearms; for it to be successful, water-displacing oil must be rubbed onto the blued steel.
- Corrosion control can be done using a coating to isolate the metal from the environment, such as paint. Large structures with enclosed box sections, such as ships and modern automobiles, often have a wax-based product (technically a slushing oil) injected into these sections. This may contain rust inhibiting chemicals as well as forming a barrier. Covering steel with concrete provides protection to steel by the high pH environment at the steel-concrete interface. However, if concrete covered steel does corrode, the rust formed can cause the concrete to spall and fall apart. This creates structural problems.
To prevent rust corrosion on automobiles, they should be kept cleaned and waxed. The underbody should be sprayed to make sure it is free of dirt and debris that could trap moisture. After a car is washed, it is best to let it sit in the sun for a few hours to let it air dry. In winter, or in salty conditions, cars should be washed more regularly as road salt (calcium chloride) can accelerate the rusting process.
References
See also
External links
- A Primer on Rust, thorough rust prevention and removal information
- Rust Removal and Prevention Articles
Rust Preventon and Rust proofing products for automotive, marine and ...
Rustbuster are market leaders in both the treatment and rust prevention rust protection and rust proofing of rust in new cars, classic cars, buses and all forms of plant commercial ...
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Rustbuster are market leaders in both the treatment and rust prevention rust protection and rust proofing of rust in new cars, classic cars, buses and all forms of plant commercial ...
Rust - Wikipedia, the free encyclopedia
Rust is a general term for a series of iron oxides, usually red oxides, formed by the reaction of iron with oxygen in the presence of water or air moisture.
Definition: rust from Online Medical Dictionary
The Online Medical Dictionary is a searchable dictionary of definitions from medicine, science and technology.
ELECTROLYTIC RUST REMOVAL (ELECTROLYSIS)
Details of non-destructively removing rust from iron and steel artifacts using electrolysis. ... Electrolysis. By Andrew Westcott. Home Page • Rust Removal • Gin Traps ...
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Photographs and information on Puccinia tritcina which affects wheat, barley, rye and grasses.
Yellow Rust - Host Range
This disease of cereals is caused by Puccinia striiformis and different forms affect wheat and barley. Photographs and information.
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