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WCLN - Corrosion Prevention скачать в хорошем качестве

WCLN - Corrosion Prevention 10 лет назад

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WCLN - Corrosion Prevention
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WCLN - Corrosion Prevention

Knowing the causes of corrosion of iron and steel, we can take the necessary steps to minimize it. These are discussed here, along with two forms of cathodic protection that are commonly used to prevent or minimize corrosion: using a sacrificial anode, and using an impressed current. http://www.BCLearningNetwork.com. 0:02corrosion of Steel which consists mainly 0:05of iron is a major problem in our 0:08society but steps can be taken to 0:10prevent it causes approachin of iron and 0:14the factors that increase it were 0:16outlined in the previous video corrosion 0:18its causes knowing these will help us 0:21find ways to prevent corrosion corrosion 0:24of iron or rusting is primarily caused 0:27by exposure of an iron surface to oxygen 0:30and water we can deal with this by 0:33painting the surface or coating it with 0:35an antitrust coding and keeping it dry 0:38painted steel objects like bridges and 0:40vehicles must be repainted periodically 0:43to maintain a continuous coding when 0:45cracks and paint occur moisture can 0:47collect and resting can take place quite 0:50rapidly another cause of corrosion of 0:53iron or steel is exposure to any 0:56stronger oxidizing agent than fe2 plus 0:58this includes all the species above fe2 1:02plus on the left side of the reduction 1:04table 1:05so we must do what we can to eliminate 1:07exposure of iron or steel objects to 1:10these oxidizing agents another potential 1:13problem is galvanic corrosion this is 1:16where iron or steel is attached to a 1:19metal higher than iron on the reduction 1:21table or less active metal in the 1:24presence of an Electra late 1:26we must be careful not to attach iron or 1:29steel to a less active metal such as an 1:31alloy containing copper when an 1:34electrolyte is present for example we 1:36must pay attention to what type of bolts 1:38or fasteners we use when building steel 1:41structures 1:42corrosion of iron arresting is enhanced 1:45by the presence of acids 1:48so we can limit resting by keeping acids 1:51away from iron or steel objects 1:53this would include protection of the 1:55objects from acid ring when the surface 1:58of an iron or steel object is exposed to 2:01an electrolyte like saltwater resting 2:03will be enhanced it can be slowed down 2:06or prevented by avoiding exposure to 2:09salt water and other electrolytes road 2:11salt should be washed off vehicles when 2:14possible also protective coatings can be 2:17used on vehicles 2:19finally when some factors are causing 2:21rusting to occur having higher 2:23temperatures can make it happen faster 2:26so when it is possible to do so we try 2:29to keep exposed iron and steel objects 2:31relatively cool 2:33another method that is widely used to 2:35prevent corrosion of iron is called 2:38cathodic protection this first type of 2:40cathodic protection will look at uses 2:43what is called the sacrificial an old 2:45this type of cathodic protection is 2:49achieved by attaching a metal that is 2:51below iron in the reduction table to the 2:54iron or steel we're trying to protect 2:56some metals we could use for this or 2:58chromium zinc manganese aluminum or 3:03magnesium 3:05it would not be practical to use these 3:07metals below magnesium on the table they 3:10react rapidly with water to form 3:11hydrogen gas metals below iron on the 3:14right side of the table are stronger 3:17reducing agents than iron which means 3:20they're more easily oxidized iron 3:22remember oxidation potentials of these 3:25are just these values with their signs 3:27switched so the oxidation potentials of 3:30these metals are all positive notice 3:32that as we move down there oxidation 3:35potential is increased from $PERCENT 3:37positive . 45 volts for iron deposit of 3:402.37 volts for magnesium notice that 3:44these metals below iron all have higher 3:47oxidation potentials than iron 3:50which means they all oxidized more 3:53readily than iron 3:55so if any of these are present with iron 3:58and an oxidizing agent like oxygen 4:00appears these will oxidize instead of 4:03the iron thus saving the iron from 4:05oxidation let's look at an example 4:06recall from the video on the causes of 4:09corrosion that when an iron surface is 4:11exposed to water and oxygen and iron 4:14atom oxidizes to form an iron two-plus 4:17cation which dissolves in the water and 4:20the electrons produced travel through 4:22the metal the equation for this 4:24oxidation is Fe solid gives fe2 plus 4:26plus two electrons 4:29this is the an old region oxygen from 4:32the air then comes in contact with the 4:34edge of the water droplet on the iron 4:36metal surface and it combines with water 4:39and the electrons form by the oxidizing 4:41iron to produce hydroxide eyes 4:44because reduction of oxygen takes place 4:47here this is called the cathode region 4:50so the anode region in the Catholic 4:52region are both on the Iron the anode is 4:55the place where iron is being oxidized 4:58to fe 2 plus and giving off electrons

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