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Questions and Answers
What is the primary reason why noble metals are resistant to corrosion?
What is the primary reason why noble metals are resistant to corrosion?
- They are highly reactive
- They are pure metals
- They are highly strained
- They have a low reactivity (correct)
What is the result of the oxidation reaction during the electrochemical process of corrosion?
What is the result of the oxidation reaction during the electrochemical process of corrosion?
- The metal remains neutral
- The metal releases electrons (correct)
- The metal gains electrons
- The metal becomes more strained
Which of the following factors does not affect the rate of corrosion?
Which of the following factors does not affect the rate of corrosion?
- Magnetic properties of metal (correct)
- Presence of electrolyte
- Surface area of metal
- Reactivity of metal
What is the product of the rusting of Iron?
What is the product of the rusting of Iron?
What is the role of the anode in the electrochemical process of corrosion?
What is the role of the anode in the electrochemical process of corrosion?
Why does corrosion occur more readily at cuts and bends in a metal?
Why does corrosion occur more readily at cuts and bends in a metal?
What is the effect of a higher temperature on the rate of corrosion?
What is the effect of a higher temperature on the rate of corrosion?
What is the role of moisture in the corrosion process?
What is the role of moisture in the corrosion process?
Which of the following is an example of an electrolyte that can enhance corrosion?
Which of the following is an example of an electrolyte that can enhance corrosion?
What is the pH range in which corrosion is more likely to occur?
What is the pH range in which corrosion is more likely to occur?
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Study Notes
What is Corrosion?
- Corrosion is a natural, irreversible process where pure metal (except noble metals) is converted into chemically stable compounds like oxides, sulfides, hydroxides, and carbonates.
- It's a slow deterioration of metal due to atmospheric gases, resulting in the formation of more stable compounds.
Common Example of Corrosion
- Rusting of Iron (Fe2O3.xH2O) is the most common corrosion.
Factors Affecting Corrosion
- Reactivity of metal: More reactive metals corrode more readily.
- Strain in metal: Corrosion occurs readily at cuts and bends in metal.
- Presence of impurities: Impurities in pure metal increase the likelihood of corrosion.
- Presence of electrolyte: Saline water (electrolyte) accelerates corrosion.
- Air and moisture: Rusting of Iron is a classic example.
- pH: Acidic mediums (pH < 7) are more corrosive than basic or neutral mediums.
- Temperature: Higher temperatures increase the rate of corrosion.
Electrochemical Theory of Corrosion (Wet Theory of Corrosion)
- Metals exposed to air, moisture, soil, etc. undergo corrosion through an electrochemical process.
- Separate anode and cathode areas form on the metal surface.
- Corrosion occurs at anodic areas through oxidation reactions, releasing electrons.
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