Ultimate Corrosion Quiz: Trivia!
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Questions and Answers
- 1.
Corrosion is a chemical reaction that involves:
- A.
The inside of the object changing from an element to a compound
- B.
The surface of the object changing from an element to a compound
- C.
Nothing happens
- D.
The surface of the object changes from one element into another element.
Correct Answer
B. The surface of the object changing from an element to a compoundExplanation
For example, Iron metal changes from Fe --> Fe2+ ionsRate this question:
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- 2.
Rusting is a special term, given to the corrosion of which metal.
- A.
Zinc
- B.
Copper
- C.
Nickel
- D.
Iron
Correct Answer
D. IronExplanation
Rusting is a special term given to the corrosion of iron because iron readily reacts with oxygen in the presence of water or moisture to form iron oxide, commonly known as rust. This process leads to the degradation and weakening of iron structures over time. Zinc, copper, and nickel also undergo corrosion, but they do not specifically refer to the term "rusting."Rate this question:
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- 3.
What conditions are required for rusting to take place?
- A.
Water only
- B.
Oxygen only
- C.
Water and oxygen
- D.
Water and carbon dioxide
Correct Answer
C. Water and oxygenExplanation
water and oxygen (from the air) are required for rusting.Rate this question:
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- 4.
Corrosion is an example of
Correct Answer
oxidationExplanation
Corrosion is a chemical process in which a material, usually a metal, reacts with its environment and undergoes oxidation. Oxidation refers to the loss of electrons by a substance, resulting in an increase in its oxidation state. In the case of corrosion, the metal atoms lose electrons and form metal ions, which then combine with oxygen in the environment to form metal oxides. This process is a classic example of oxidation, as it involves the loss of electrons by the metal.Rate this question:
- 5.
What effect does salt have on the rate of corrosion?
- A.
No effect
- B.
Speeds up corrosion
- C.
Slows down corrosion
Correct Answer
B. Speeds up corrosionExplanation
Salt acts as an electrolyte and speeds up corrosion.Rate this question:
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- 6.
Which of the following is not an example of physical protection?
- A.
Greasing
- B.
Painting
- C.
Attaching the metal to the negative terminal of a battery
- D.
Electroplating
- E.
Galvanising
Correct Answer
C. Attaching the metal to the negative terminal of a batteryExplanation
The other 2 types of physical protection are tin-plating and coating with plastic. Physical protection puts a layer between the metal and water/oxygen.Rate this question:
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- 7.
Which of the following metals would protect iron by electrons flowing to the iron?
- A.
Magnesium
- B.
Silver
- C.
Tin
- D.
Copper
Correct Answer
A. MagnesiumExplanation
magnesium is higher that iron in the electrochemical series. It will protect the iron by sacrificing itself to protect the iron. electrons will flow from Mg --> FeRate this question:
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- 8.
When objects (gates) are galvanized, what metal is used to protect the iron.
- A.
Aluminium
- B.
Copper
- C.
Nickel
- D.
Zinc
Correct Answer
D. ZincExplanation
Galvanising is covering with a layer of zinc.Rate this question:
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- 9.
What type of protection is galvanizing?
- A.
Physical protection
- B.
Sacrificial protection
- C.
Physical and sacrificial protection
- D.
None of the above.
Correct Answer
C. Physical and sacrificial protectionExplanation
Covering with a layer of zinc, excludes water/oxygen - physical protection, Zinc is higher that iron in the Electrochemical series, so it will corrode to protect the iron (Sacrificial protection)Rate this question:
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- 10.
Rusting of iron is a typical example for
- A.
Chemical corrosion
- B.
Electrochemical corrosion
- C.
Physical reaction
- D.
None of these
Correct Answer
B. Electrochemical corrosionExplanation
Rusting of iron is a typical example of electrochemical corrosion because it involves a chemical reaction between iron, water, and oxygen. This reaction occurs in the presence of an electrolyte, such as water, which allows for the flow of electric current. The iron acts as the anode, where it undergoes oxidation and loses electrons, while oxygen acts as the cathode, where it undergoes reduction and gains electrons. This electrochemical process leads to the formation of iron oxide, commonly known as rust. Therefore, electrochemical corrosion is the correct explanation for the rusting of iron.Rate this question:
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- 11.
The pitting factor of unity represents ____ corrosion.
- A.
Uniform
- B.
Galvanic
- C.
Inter granular
- D.
Fretting
Correct Answer
A. UniformExplanation
The pitting factor of unity represents uniform corrosion. This means that the corrosion occurs evenly across the surface, causing a uniform loss of material. This type of corrosion is characterized by the formation of pits or craters that are relatively evenly distributed. It is often caused by the exposure of a metal to a corrosive environment, such as exposure to moisture or chemicals. In contrast, other types of corrosion, such as galvanic or intergranular corrosion, occur in a non-uniform manner and may result in localized areas of damage.Rate this question:
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- 12.
Passivity in stainless steel is due to the formation of?
- A.
Sulphide film
- B.
Carbide film
- C.
Oxide film
- D.
Chloride film
Correct Answer
C. Oxide filmExplanation
Passivity in stainless steel is due to the formation of an oxide film. This film acts as a protective layer on the surface of the steel, preventing further corrosion and degradation. The oxide film is formed when the steel is exposed to oxygen in the atmosphere, and it is this film that gives stainless steel its corrosion-resistant properties. The oxide film is stable and adheres tightly to the surface of the steel, providing a barrier against corrosive elements.Rate this question:
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- 13.
An iron pipe carrying water is more anodic to copper. This is due to:
- A.
Concentration cell
- B.
Galvanic cell
- C.
Electrolytic cell
- D.
Leclanche cell
Correct Answer
B. Galvanic cellExplanation
The correct answer is Galvanic cell. In a galvanic cell, two different metals are in contact with an electrolyte solution, creating a potential difference. In this case, the iron pipe and copper are in contact with water, creating a galvanic cell. The iron pipe, being more anodic, will undergo oxidation and corrode more readily compared to the copper. This is because iron has a higher tendency to lose electrons and undergo oxidation reactions.Rate this question:
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- 14.
Which of the following metal can be used for cathodic protection of steel?
- A.
Al
- B.
Cu
- C.
Ag
- D.
Au
Correct Answer
A. AlExplanation
Aluminum (Al) can be used for cathodic protection of steel. Cathodic protection is a technique used to prevent corrosion of a metal surface by making it the cathode of an electrochemical cell. In this process, a more active metal is connected to the steel, which acts as the anode and corrodes instead. Aluminum is commonly used for this purpose because it is more active than steel, meaning it will corrode preferentially, protecting the steel from corrosion. Copper (Cu), silver (Ag), and gold (Au) are not suitable for cathodic protection of steel.Rate this question:
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- 15.
In zinc – aluminium galvanic couple, when exposed to acidic solutions.
- A.
Zinc dissolves
- B.
Aluminium dissolves
- C.
Both dissolve
- D.
None of these
Correct Answer
A. Zinc dissolvesExplanation
In a zinc-aluminium galvanic couple, when exposed to acidic solutions, the zinc dissolves. This is because zinc is more reactive than aluminium, and in the presence of acid, it undergoes oxidation and forms zinc ions, which then dissolve into the solution. Aluminium, on the other hand, is less reactive and does not dissolve in acidic solutions. Therefore, the correct answer is zinc dissolves.Rate this question:
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- 16.
Typical example for anodic metallic coating is:
- A.
Zn on Steel
- B.
Cu on Steel
- C.
Au on steel
- D.
All of these
Correct Answer
A. Zn on SteelExplanation
Anodic metallic coating refers to a process where a metal is used as a sacrificial anode to protect the base metal from corrosion. In this case, Zn (zinc) is applied on steel as a coating. Zinc is more reactive than steel, so it acts as a sacrificial layer, corroding in place of the steel. This helps to protect the steel from rusting and extends its lifespan. Therefore, the correct answer is Zn on Steel.Rate this question:
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- 17.
Pourbaix diagram is a graphical plot of?
- A.
E Vs pH
- B.
E Vs Log i
- C.
E Vs time
- D.
Current Vs Potential
Correct Answer
A. E Vs pHExplanation
A Pourbaix diagram is a graphical plot that shows the stability of different chemical species in a solution as a function of both the electrode potential (E) and the pH of the solution. It helps to determine the thermodynamically stable regions for different chemical reactions and species in an electrochemical system. By plotting E vs pH, the Pourbaix diagram provides valuable information about the stability of different compounds and the conditions under which they can exist.Rate this question:
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- 18.
When a non-metallic material forms a crevice on the metallic surface it is known as?
- A.
Pitting
- B.
Gasket
- C.
Uniform
- D.
Fretting
Correct Answer
B. GasketExplanation
A gasket is a non-metallic material that is used to create a seal between two surfaces. In this context, when a non-metallic material forms a crevice on a metallic surface, it can be referred to as a gasket. The other options, such as pitting, uniform, and fretting, do not accurately describe the situation described in the question.Rate this question:
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- 19.
Which of the following can be used to prevent rusting?
- A.
Paint
- B.
Zinc
- C.
None of the above
- D.
All of the above
Correct Answer
D. All of the aboveExplanation
All of the above options can be used to prevent rusting. Paint forms a protective barrier between the metal and the surrounding environment, preventing direct contact with moisture and oxygen. Zinc can be used as a sacrificial coating, where it corrodes instead of the metal, protecting it from rust. Therefore, both paint and zinc can effectively prevent rusting.Rate this question:
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- 20.
Iron can be corroded easily.
- A.
True
- B.
False
Correct Answer
A. TrueExplanation
Iron can be corroded easily because it is a reactive metal. When iron comes into contact with oxygen and moisture, it undergoes a chemical reaction known as oxidation, forming iron oxide, commonly known as rust. This process weakens the iron and causes it to deteriorate over time. Therefore, iron is susceptible to corrosion and can be easily corroded if not properly protected.Rate this question:
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- 21.
Corrosion is a:
- A.
Chemical change
- B.
Disaster
- C.
Physical change
- D.
None of the above
Correct Answer
A. Chemical changeExplanation
Corrosion is considered a chemical change because it involves a reaction between a metal and its environment, usually oxygen or moisture. This reaction leads to the formation of new compounds, such as metal oxides or metal hydroxides, which have different properties than the original metal. This process is irreversible and results in the deterioration and degradation of the metal over time. Therefore, corrosion is classified as a chemical change rather than a physical change or a disaster.Rate this question:
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- 22.
Can corrosion be helpful?
- A.
True
- B.
False
Correct Answer
B. FalseExplanation
Corrosion is a destructive process that occurs when metals react with their environment, leading to the deterioration of the metal. It causes damage to structures, equipment, and objects, making it generally considered as harmful. Therefore, corrosion is not helpful.Rate this question:
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- 23.
Describe why Ecorr shifts to more negative when a cathodic inhibitor is used:
- A.
Because only anodic reaction is controlled the reactions.
- B.
Because only cathodic reaction is controlled the reactions.
Correct Answer
A. Because only anodic reaction is controlled the reactions.Explanation
Because only anodic reaction is controlled the reactions.Rate this question:
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