describe the conditions under which corrosion of metals occurs?

Answer 1

oxidation, as in rusting.

Answer 2

It is the loss of an electron of metals reacting with water or oxygen. Weakening of iron due to oxidation of the iron atoms is an example of electrochemistry, when certain metals are exposed to certain chemicals, they 'burn'. When iron is exposed to water and oxygen, it rusts (or corrodes), which is an electrical reaction of electron transfer. Rust is actually iron burning very, very slowly.
Some metals corrode much faster than others. A hunk of zinc is attached to natural gas pipe, because zinc corrodes so much faster. than steel pipe. This is called sacrificial corrosion protection. There is also something called active corrosion protection, where an electrical source is applied to metal to drive away the corrosion process.
Copper corrodes faster than lead - so if you put a penny under the leads to your car battery, the pennys will corrode before the posts. All the wire conections stay clean from corrosion (until the penny cannot corrode any further, then you need to change the penny.

Answer 3

First i ask your self what test you're talking approximately. did you be responsive to that the act of "viewing" specific quantum mechanic experiments motives a metamorphosis in effects. that may not great organic it particularly is technological information. be chuffed to digital mail me. i'm curious what experiments you're touching on

Answer 4

When the presence of air and water are in contact with unprotected surfaces

Answer 5

It depends on the environment. pH is related to, but not synonymous with, hydrogen concentration or amount of acid. Can you be more specific?