made cathode
made anode
used with a metal of lower electropositive potential
initially coated with tin
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The most effective method of preventing corrosion in iron is the cathodic protection.
By this method, a more electropositive (or more reactive) metal (e.g. Zn or Mg) is made the anode and the iron, the cathode. A conducting wire is connected between them. Thus, the iron is prevented from going into solution as Fe2+, i.e. the reaction:
Fe(s) → Fe2+(aq) + 2e-(aq) is prevented from taking place.
I.e. Anodic reaction: Zn(s) → Zn2+(aq) + 2e-(aq)
Cathodic reaction: Fe2+(aq) + 2e-(aq) → Fe(s)
The question says: “In an electrolytic setup to protect iron from corrosion, the iron is…”
First, what is this question really asking?
It’s basically about how to stop iron from rusting using electricity. There’s a trick here: rusting is a type of chemical reaction called oxidation. Rust happens when iron loses electrons and reacts with oxygen and water. So if we can stop iron from losing electrons, it won’t rust.
Now, they mention “electrolytic setup.” Don’t freak out. Electrolytic just means we’re using electricity to drive a chemical reaction that normally wouldn’t happen by itself. In this case, the reaction we’re controlling is corrosion.
In any electrolytic cell, there are two electrodes:
Anode – the electrode where oxidation happens. Things lose electrons here.
Cathode – the electrode where reduction happens. Things gain electrons here.
Now remember: rusting is iron losing electrons. So iron rusts if it becomes an anode. That’s exactly what happens naturally.
So, if you want to protect iron from corrosion, you need to make sure iron does not lose electrons. That means iron must become the cathode, because at the cathode, electrons are being given to it, not taken from it. If iron is the cathode, it is safe from rusting.
So option A) made cathode is already sounding correct.
Let’s quickly look at the other options so you can see why they are wrong:
B) made anode – This is the opposite of what we want. If iron is the anode, it will corrode faster because it will lose electrons. That’s literally the rusting process. Wrong.
C) used with a metal of lower electropositive metal – This is a bit tricky because it’s talking about something called sacrificial protection. You sometimes attach a metal that’s more “eager” to lose electrons, like zinc. That metal will corrode instead of iron. But in an electrolytic setup, we are controlling the electrodes with electricity, not just attaching a metal. So this is not the primary method they are testing here.
D) initially coated with tin – This is called galvanization. It works in real life because tin protects iron from water and oxygen. But this is a mechanical coating method, not an electrolytic method. The question specifically says “electrolytic setup,” so this is a trap.
So the correct answer is A) made cathode.
The correct answer is A.Because the metal used for electroplating is made the anode while the object to be electroplated is made the anode.Pls kindly make a correction to the answer.
Electrolytic protection is a method used to prevent corrosion of metals. In this method, the metal to be protected is connected to the negative terminal of a DC power supply and made the cathode. A more reactive metal, called the sacrificial anode, is connected to the positive terminal of the power supply and made the anode.
When the power supply is switched on, the sacrificial anode is oxidized instead of the protected metal. The sacrificial anode corrodes, and its metal ions go into the solution, while the protected metal (iron in this case) gains electrons from the cathode, which slows down or prevents its corrosion. This is because the metal ions from the anode react with the electrons from the cathode to form a non-corrosive layer on the surface of the iron.
So, in the given electrolytic set-up to protect iron from corrosion, the iron is made cathode so that it gains electrons and reduces the rate of corrosion
to prevent iron from rusting it is made the cathode ...but in the process of coating metals to prevent them from corroding u make use of metal above it in the electrochemical series making it the cathode and the metal to be plated the anode ...correct option b
.........reference to lamlad chemistry
