Does iron rust faster in water or bleach?

Answer 1

Rust is essentially oxidation, or a chemical interaction involving oxygen. When oxidation occurs in some elements, a thin film is formed as a result--such as the green layer that copper acquires. Other elements, such as iron, show rust as evidence of oxidation. If iron--or metal related to iron--is exposed to an environment both oxygen-rich and friendly toward the catalyst, then the oxidation process will begin. Molecules of iron at the surface of the iron object will exchange atoms with the oxygen in the air, and what atoms are left will form a new substance, the reddish-brown rust.

Oxidation is an electrochemical process that acts somewhat like a battery, exchanging small amounts of electricity. Like batteries, a solution helps this process by allowing electrons to move more easily between the two elements, and also like batteries, different solutions work better than others. Water takes some of the atoms and changes them into a light form of acid as the oxidation process continues, which helps metal rust even faster.

This acidic transformation occurs with pure water, but when the water is already salty it starts out as a minor acid and becomes an even more powerful electrolyte, facilitating the rusting process. There is then a hierarchy in the rust process. Rust does not easily form in dry climate, but in a wet climate the oxygen can access the metal more easily through the water vapor, and rust occurs much faster. Pure water forms an acidic solution and allows the oxidation process to happen more easily, and salty water works even better since it is already a catalyst. Prime rust conditions occur when the metal is regularly exposed to salt water and air

Answer 2

A bleach is a chemical that removes color or whitens, often via oxidation. Common chemical bleaches include household "chlorine bleach", a solution of approximately 3-6% sodium hypochlorite (NaOCl).
"Rusting", is an oxidization process. Taking iron rusting for example, ion atoms would loose 2 electrons, or to be oxidized, to becomes iron ions:
Fe(s) → Fe2+(aq) + 2e−
The iron ions may react with some thing further to form precipitates. Reaction in the opposite direction of oxidation is called reduction:
Fe2+(aq) + 2e− → Fe(s), −0.44v
To indicate the easiness or hardness of the oxidation/reduction process, people use so-called "Standard Reduction Potentials", like the number -0.44v at the end of reduction equation above, to show how it is. The more negative the number is, the easier it is to be oxidized and the harder it is to be reduced (back to metal). Vice versa, the more positive the number is, the harder it is to be oxidized and the easier it is to be reduced.
For non-metal element, we also can assign the standard reduction potential such as:
2HClO(aq) + 2H+ + 2e− → Cl2(g) + 2H2O, +1.63V
Cl2(g) + 2e− → 2Cl−(aq) +1.36V
2H+(aq) + 2e− → H2(g), 0.00V
This indicate that bleach (+1.63V) is easy to be reduced, thus it would grab the electrons from something else. That is to say, it is a strong oxidizer to cause other metals to be oxidized. Even Cl2 formed as product still serves as a strong oxidizer (+1.36V). On the other hand, water, containing small amount of H+, is extremely weak oxidizer (with reduction potential of 0.00V).
This explains why iron rust much quick in bleach than in water.