Rusting is a reduction process
Rusting of iron takes place in the presence of oxygen and moisture
the rust formed is reddish brown
the major constituent of rust is hydrated iron (lll) oxide
rusting is similar to burning
Explanation
No explanation available
Video Explanation
No video available
Post your Contribution
Discussions (3)
Explanation
Log In
SPONSORED: Preparing to Sit for an Exam? Study and Practice with Ulearngo
Home » Past Questions » Chemistry » Which of the following is not true of the rusting of iron?
Which of the following is not true of the rusting of iron?
ChemistryWAEC SSCE
Question
Which of the following is not true of the rusting of iron?
Options
A)
Rusting is a reduction process
B)
Rusting of iron takes place in the presence of oxygen and moisture
C)
the rust formed is reddish brown
D)
the major constituent of rust is hydrated iron (lll) oxide
E)
rusting is similar to burning
Related Lesson: Standard Reduction Potentials | Electrochemistry
The correct answer is A.
Explanation:
Rusting is a chemical process that occurs when iron or steel reacts with water and oxygen to form a new substance called rust (hydrated iron (III) oxide). This process is an example of corrosion. It is an oxidation process, not a reduction process, which directly contradicts Option A, making it the correct answer.
Let's understand this a bit more. In chemistry, oxidation and reduction reactions often occur simultaneously, and they are collectively known as redox reactions. Oxidation refers to the loss of electrons during a reaction by a molecule, atom or ion, while reduction refers to the gain of electrons. In the case of rusting, iron (Fe) loses electrons to form iron (III) ions (Fe3+), which is an oxidation process.
Oxidation:
The oxygen in the air gains these electrons and is reduced to form hydroxide ions (OH-).
Reduction:
These ions then react with each other to form hydrated iron (III) oxide (Fe2O3.H2O), which is rust. This reddish-brown substance gives rusted iron its characteristic color, confirming Options C and D.
Rusting indeed requires both oxygen and water, as stated in Option B. This is why iron rusts faster in humid or marine (sea-side) environments where moisture is abundant.
Lastly, Option E suggests that rusting is similar to burning. While both processes are types of oxidation reactions, they occur at very different rates. Burning is a rapid form of oxidation that releases light and heat, whereas rusting is a slow form of oxidation that does not release light or heat.
The correct answer is A.
Explanation:
Rusting is a chemical process that occurs when iron or steel reacts with water and oxygen to form a new substance called rust (hydrated iron (III) oxide). This process is an example of corrosion. It is an oxidation process, not a reduction process, which directly contradicts Option A, making it the correct answer.
Let's understand this a bit more. In chemistry, oxidation and reduction reactions often occur simultaneously, and they are collectively known as redox reactions. Oxidation refers to the loss of electrons during a reaction by a molecule, atom or ion, while reduction refers to the gain of electrons. In the case of rusting, iron (Fe) loses electrons to form iron (III) ions (Fe3+), which is an oxidation process.
Oxidation:
The oxygen in the air gains these electrons and is reduced to form hydroxide ions (OH-).
Reduction:
These ions then react with each other to form hydrated iron (III) oxide (Fe2O3.H2O), which is rust. This reddish-brown substance gives rusted iron its characteristic color, confirming Options C and D.
Rusting indeed requires both oxygen and water, as stated in Option B. This is why iron rusts faster in humid or marine (sea-side) environments where moisture is abundant.
Lastly, Option E suggests that rusting is similar to burning. While both processes are types of oxidation reactions, they occur at very different rates. Burning is a rapid form of oxidation that releases light and heat, whereas rusting is a slow form of oxidation that does not release light or heat.
