Corrosion std 12 ch 3l RUSTING OF IRON l GALVANIZATION
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1) Rusting is the corrosion of iron caused by a reaction with oxygen and moisture in the air. 2) The rusting process is electrochemical, where iron acts as the anode and is oxidized, releasing electrons, while oxygen is reduced at the cathode. 3) Factors that affect rusting include moisture content, the purity and type of metal, amount of impurities, and presence of electrolytes that allow conduction of ions involved in the corrosion reaction.
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There are three main varieties of iron based on carbon content: cast iron contains 2-5% carbon and is the impure form used to make steel and wrought iron; wrought iron contains 0.12-0.25% carbon and is the purest form used for chains and magnet cores; steel contains 0.1-1.5% carbon and has properties dependent on carbon content, used for many applications. Rusting of iron occurs via an electrochemical process where iron acts as the anode, releasing electrons and ferrous ions while hydrogen ions are reduced to hydrogen gas at cathode sites on the metal surface. The ferrous ions further oxidize to ferric oxide which absorbs moisture from the
Corrosion-Dr. Surendran Parambadath
This document discusses corrosion and how it affects metals. It defines corrosion as the slow process of decay of metals due to chemical or electrochemical reaction with their environment. This causes the formation of compounds like oxides on the metal surface. Corrosion occurs through both dry chemical reactions and wet electrochemical reactions that set up galvanic cells. The rate of corrosion is affected by factors like the metal's position in the galvanic series, purity, environment, and characteristics of the corrosion products formed. Common types of corrosion discussed are rusting of iron and methods to prevent or reduce corrosion like coatings, cathodic protection, and modifying the environment.
Corrosion ppt part 1
The document discusses corrosion of metals and its various types. It defines corrosion as the deterioration of metal due to chemical reactions with the environment. Corrosion occurs via oxidation and causes metal loss. The main factors influencing corrosion are the metal composition, environmental chemicals, temperature, and design. Corrosion can be uniform, galvanic, pitting, intergranular or stress-related. Electrochemical corrosion involves the formation of anodes and cathodes on a metal surface.
Corrosion
The document discusses corrosion and rusting of metals like iron. Rust is a hydrated ferric oxide that forms when iron is exposed to oxygen and moisture in the air. The rusting process occurs via an electrochemical reaction where iron acts as an anode and donates electrons, forming ferrous ions. These then react with oxygen and hydroxyl ions to form rust. Methods to prevent rusting include using barriers like paint or galvanization where a more reactive metal like zinc protects the iron.
Corrosion & Mechanism of Dry corrosion
1. Dry or chemical corrosion occurs via direct chemical reaction between a metal surface and gases in the atmosphere like oxygen, carbon dioxide, hydrogen sulfide, and sulfur dioxide. It involves adsorption of gas molecules on the metal surface.
2. The mechanism of dry corrosion involves oxidation of the metal surface and reduction of gas molecules, forming a metal oxide layer. The nature and properties of this oxide layer determines whether it is protective or porous.
3. According to the Pilling-Bedworth rule, a protective oxide layer has a volume equal to or greater than the original metal, while a porous layer has a smaller volume, allowing further corrosion. Metals like chromium and aluminum form protective passive layers contributing to corrosion resistance.
Chemistry review c10 c14
1. The document discusses various properties and reactions involving metals and non-metals. It describes the structure of alloys and how they are stronger than pure metals.
2. Key extraction methods are related to a metal's position in the reactivity series, such as electrolysis of reactive metals and blast furnaces for less reactive metals.
3. Common uses of metals such as aluminum, zinc, and iron alloys are explained in terms of the metals' properties including strength, corrosion resistance, and galvanization.
Blast furnace presentation
The blast furnace is a counter-current heat exchanger used to smelt iron from iron ore for steel production. Reactions inside reduce iron oxides to molten iron and separate impurities into a slag. The furnace operates at over 1500°C, using coke as the reducing agent and limestone as a flux. Key reactions include the reduction of iron oxides to iron and carbon monoxide, and the removal of impurities like sulfur. The process produces molten iron, known as pig iron, and a slag byproduct. The composition of the pig iron depends on the burden chemistry and furnace operating temperature.
CORROSION ENGINEERING.pptx
This document discusses corrosion engineering and provides details on various corrosion topics. It begins with an introduction to corrosion and defines it as the deterioration of metal through chemical or electrochemical reactions with the environment. Some key points covered include:
- Corrosion costs the US economy $300 billion per year. Common examples of corrosion are rusting of iron when exposed to air and the formation of a green or blue film on copper in moist air.
- An electrochemical cell converts chemical energy of an indirect redox reaction into electrical energy. During corrosion, the metal being corroded acts as the anode and loses electrons/dissolves while another metal acts as the cathode and gains electrons.
- The main types of corrosion
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We present the JWST discovery of SN 2023adsy, a transient object located in a host galaxy JADES-GS
+
53.13485
−
27.82088
with a host spectroscopic redshift of
2.903
±
0.007
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) despite a host galaxy with low-extinction and has a high Ca II velocity (
19
,
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,
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km/s) compared to the general population of SNe Ia. While these characteristics are consistent with some Ca-rich SNe Ia, particularly SN 2016hnk, SN 2023adsy is intrinsically brighter than the low-
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Ca-rich population. Although such an object is too red for any low-
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Ca-rich SNe Ia, SN 2023adsy is standardizable and gives no indication that SN Ia standardized luminosities change significantly with redshift. A larger sample of distant SNe Ia is required to determine if SN Ia population characteristics at high-
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Signatures of wave erosion in Titan’s coasts
The shorelines of Titan’s hydrocarbon seas trace flooded erosional landforms such as river valleys; however, it isunclear whether coastal erosion has subsequently altered these shorelines. Spacecraft observations and theo-retical models suggest that wind may cause waves to form on Titan’s seas, potentially driving coastal erosion,but the observational evidence of waves is indirect, and the processes affecting shoreline evolution on Titanremain unknown. No widely accepted framework exists for using shoreline morphology to quantitatively dis-cern coastal erosion mechanisms, even on Earth, where the dominant mechanisms are known. We combinelandscape evolution models with measurements of shoreline shape on Earth to characterize how differentcoastal erosion mechanisms affect shoreline morphology. Applying this framework to Titan, we find that theshorelines of Titan’s seas are most consistent with flooded landscapes that subsequently have been eroded bywaves, rather than a uniform erosional process or no coastal erosion, particularly if wave growth saturates atfetch lengths of tens of kilometers.
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SDSS1335+0728: The awakening of a ∼ 106M⊙ black hole⋆
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Corrosion std 12 ch 3l RUSTING OF IRON l GALVANIZATION
- 1. CORROSION STD 12 SCI ( E ) CHAPTER-3 – ELECTROCHEMISTRY BY :- MS. MAYRI R SOMPURA HJD INSTITUTE KERA-KUTCH
- 2. CORROSION Deterioration of the metal ( physical properties ) Copper – green covering Aluminum and silver – greyish black spots Iron – reddish brown spots
- 3. • it is because of the exposure of iron surface to the atmospheric gases and moisture. • It is a reddish brown powder- RUST Fe2O3.X H2O RUSTING OF IRON
- 4. ELECTROCHEMICAL THEORY OF RUSTING:- • Atmospheric gases:- • CO2 + H2O → H2CO3 • Ionization of H2CO3:- • H2CO3 → 2H+ + CO-2 3 • Anode (oxidation) • 2 Fe → 2 Fe+2 + 4 e- • Cathode (reduction) • 4 H+ + O2 + 4 e- → 2H2O • RUSTING :- • 2 Fe+2 + 4 H2O + O2 → Fe2O3 • Fe2O3 + X H2O → Fe2O3.X H2O
- 5. FACTORS AFFECTING RUSTING :- • Moisture content in atmosphere. • Nature of metal. Impure iron rusts fast Pure iron do not rust fast • Amount of impurities • Amount of electrolytes present. • More reactive the metal more readily it corrodes ( forming metal oxides on the surface)
- 6. PREVENTION OF CORROSION :- • Grease oil lubrication • Anti rust solution • Barrier method – GALVANIZATION • Galvanization is covering iron metal surface with a layer of zinc. • Can also be coated by less electropositive metal like tin (Sn). Zinc readily reacts with atmospheric oxygen. Hence zinc gets oxidized and it depleates eventually and iron remains safe.