.....3 METHODS OF APPLYING CATHODIC PROTECTION........................................5 3.1 3.2 4 4.1 4.2 4.3 4.4 4.5 4.6 4.7 IMPRESSED CURRENT..........................................................................................5 SACRIFICIAL ANODES..........................................................................................6 PROTECTION POTENTIALS .................................................................................8 CURRENT DENSITY...................................
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For that we have learned and studied these contents. I will concisely review about that. first‚ The structure of OLED is actually pretty simple. it consists sandwiched organic films between anode and cathode. principle is that Excitons are generated by electrons from cathode‚ holes from anode. when its fall down to ground state‚ energy release as the form of photon. at that time‚ OLEDs emit light. these are making process of oled. after etching cleaning and drying ITO‚ we operate
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because it helps demonstrate how the galvanic cells that make up a car battery work. Some batteries use galvanic cells to transfer chemical energy into electric energy. They depend on two metals‚ a cathode or positive terminal (such as copper) and an anode or negative terminal (such as zinc). These are placed in an electrically conductive solution that allows ions to travel freely between the two metals. The solution is typically an acid. Car batteries use sulfuric acid‚ but potatoes contain phosphoric
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500V Megger. Read the relevant section in this manual before carrying out any tests. c) There is no need of protective current as far as ship is well enclosed by a good hull coating (newbuildings or just repaired ships) or the temporary sacrificial anodes around ship’s bow and stern hull area are still alive‚ which means our system dissipates no current under fully automatic control realizing ship is well protected from corrosion. Then you may see protective current when ship’s hull coating gets thinner
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TENDING MACHINE PTM is the crucial equipment of large anode pre-baking workshop. It is used in the environment of high temperature‚ large current‚ strong magnetic field and HF gas. It can perform the following procedures ANODE CHANGE: Anode in the pots is changed at an interval of every 27 days since daily 1.5 cm of the anode gets consumed. A carbon block is usually 55 cm high of which only 40 cm can be used up. The main reason behind the anode consumption is the following electrolytic reaction
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table of standard reduction potentials has been recorded so the E( values of half reactions can be accurately known and referred to. – Anode: The electrode where oxidation occurs. Electrons move away from the anode. – Cathode: The electrode where reduction occurs. Electrons are “pulled” towards the cathode. – These electrodes (anode and cathode) are linked by an external wire which enables electron flow between the two solutions. – Salt bridge: A salt bridge contains non reactive
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knowledge that will assist you in completing this assessment task: describe and explain galvanic cells in terms of oxidation/reduction reactions outline the construction of galvanic cells and trace the direction of electron flow define the terms anode‚ cathode‚ electrode and electrolyte to describe galvanic cells perform a first-hand investigation to identify the conditions under which a galvanic cell is produced perform a first-hand investigation and gather first-hand information to measure the
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The polymerase chain reaction (PCR) is a biochemical technology in molecular biology used to amplify a single copy or a few copies of a piece of DNA across several orders of magnitude‚ generating thousands to millions of copies of a particular DNA sequence. Developed in 1983 by Kary Mullis‚[1][2] PCR is now a common and often indispensable technique used in medical and biological research labs for a variety of applications.[3][4] These include DNA cloning for sequencing‚ DNA-based phylogeny‚ or
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through a wire‚ that is called a circuit. Batteries have three parts to them‚ an anode‚ a cathode‚ and an electrolyte. The cathode and the anode are hooked up to an electrical circuit. The chemical reaction that is happening causes the electrons to build up at the anode. When the circuit is closed the electrons will be able to get to the cathode. When the electrochemical process change the chemicals in the anode and cathode it makes them stop supplying electrons. So that’s why there’s a limited
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ions present in copper(II) sulphate solution. b)What would you expect to observe in Beakers A and B when a current is flowing through the circuit? c)Identify the cathode in Beaker A and the anode in Beaker B. d)Write an ionic equation to represent the reaction occurring at the cathode in Beaker A and the anode in Beaker B. e)Two industrial applications of electrolysis are purification and anodising. (i) Explain how an impure sample of copper can be purified 3.The circuit in Figure 2 can be used
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