Yes, The causes of corrosion require the presence of water and oxygen. Water can combine with carbon dioxide in the air to form carbonic acid, a weak acid.
The causes of corrosion require the presence of water and oxygen. Water can combine with carbon dioxide in the air to form carbonic acid, a weak acid.
When this acidic solution reaches iron, two reactions occur. First, the acidified water (a good electrolyte – more on this later) will dissolve some of the iron by removing electrons. Then, the water will begin to break down into hydrogen and oxygen. Free oxygen reacts with dissolved iron to form iron oxide, and iron oxide is rust.
RELATED
How to Write the Balanced Chemical Reaction for the Rusting of Iron
Updated March 26, 2020
By Rosann Kozlowski
Reviewed by: Lana Bandoim, B.S.
The silver shine of a new nail may begin to show reddish-brown spots eventually, especially when exposed to the elements for an extended amount of time. This is the familiar beginning of rusting. The causes of rusting are chemical and involve reactions with water and oxygen.
Chemical Causes of Rusting
The causes of corrosion require the presence of water and oxygen. Water can combine with carbon dioxide in the air to form carbonic acid, a weak acid.
When this acidic solution reaches iron, two reactions occur. First, the acidified water (a good electrolyte – more on this later) will dissolve some of the iron by removing electrons. Then, the water will begin to break down into hydrogen and oxygen. Free oxygen reacts with dissolved iron to form iron oxide, and iron oxide is rust.
From this explanation, a word equation for rust can be created:
Iron + water + oxygen → iron oxide (rust)
Resulting Chemical Reaction of Rust
The resulting chemical reaction of rusting is:
4Fe(s) + 3O2(g) + 6H2O(l)→ 4Fe(OH)3(s)
This porous rust, Fe(OH)3(s) reacts with additional oxygen to yield a more crystallized rust with a formula of Fe2O3 . xH20. The hydrated iron (III) oxide (Fe2O3) has water attached with approximately 3/2 H2O; the water amount is not fixed thus the x in front of the H20.
This reaction, however, happens in steps.
Electrochemical Process of Rust
Metals like iron dissolve in an electrochemical process. This means the process acts like an electrochemical cell (commonly thought of as a battery).
The anode will be a location where the metal is stressed or damaged. The cathode is another part of the metal not undergoing corrosion. Water acts as the electrolyte – the bridge – and transports ions to keep the flow of electrons moving, or, in this case, the flow of electrons that will corrode the anode area of the iron.
All electrochemical processes involve a type of chemical reaction called oxidation-reduction or redox reactions. In a redox reaction, there is a transfer of electrons. The transfer of electrons in corrosion are taken from the surface of the metal and transferred to suitable electron acceptors, like oxygen and hydrogen.
Answers & Comments
Answer:
Yes, The causes of corrosion require the presence of water and oxygen. Water can combine with carbon dioxide in the air to form carbonic acid, a weak acid.
Explanation:
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Answer:
The causes of corrosion require the presence of water and oxygen. Water can combine with carbon dioxide in the air to form carbonic acid, a weak acid.
When this acidic solution reaches iron, two reactions occur. First, the acidified water (a good electrolyte – more on this later) will dissolve some of the iron by removing electrons. Then, the water will begin to break down into hydrogen and oxygen. Free oxygen reacts with dissolved iron to form iron oxide, and iron oxide is rust.
RELATED
How to Write the Balanced Chemical Reaction for the Rusting of Iron
Updated March 26, 2020
By Rosann Kozlowski
Reviewed by: Lana Bandoim, B.S.
The silver shine of a new nail may begin to show reddish-brown spots eventually, especially when exposed to the elements for an extended amount of time. This is the familiar beginning of rusting. The causes of rusting are chemical and involve reactions with water and oxygen.
Chemical Causes of Rusting
The causes of corrosion require the presence of water and oxygen. Water can combine with carbon dioxide in the air to form carbonic acid, a weak acid.
When this acidic solution reaches iron, two reactions occur. First, the acidified water (a good electrolyte – more on this later) will dissolve some of the iron by removing electrons. Then, the water will begin to break down into hydrogen and oxygen. Free oxygen reacts with dissolved iron to form iron oxide, and iron oxide is rust.
From this explanation, a word equation for rust can be created:
Iron + water + oxygen → iron oxide (rust)
Resulting Chemical Reaction of Rust
The resulting chemical reaction of rusting is:
4Fe(s) + 3O2(g) + 6H2O(l)→ 4Fe(OH)3(s)
This porous rust, Fe(OH)3(s) reacts with additional oxygen to yield a more crystallized rust with a formula of Fe2O3 . xH20. The hydrated iron (III) oxide (Fe2O3) has water attached with approximately 3/2 H2O; the water amount is not fixed thus the x in front of the H20.
This reaction, however, happens in steps.
Electrochemical Process of Rust
Metals like iron dissolve in an electrochemical process. This means the process acts like an electrochemical cell (commonly thought of as a battery).
The anode will be a location where the metal is stressed or damaged. The cathode is another part of the metal not undergoing corrosion. Water acts as the electrolyte – the bridge – and transports ions to keep the flow of electrons moving, or, in this case, the flow of electrons that will corrode the anode area of the iron.
All electrochemical processes involve a type of chemical reaction called oxidation-reduction or redox reactions. In a redox reaction, there is a transfer of electrons. The transfer of electrons in corrosion are taken from the surface of the metal and transferred to suitable electron acceptors, like oxygen and hydrogen.