If you keep an iron piece in solid state CuSO4 crystals , does it get any reaction ? Guess the reason
What are the preventive methods do you take for rusting iron material
If n=3 ,mention the orbitals present in the shell and write maximum number of electrons in the shell
A person is unable to see distant objects , show the defect of vision of the person with the help of ray diagram
If you keep an iron piece in solid state CuSO4 crystals , does it get any reaction ? Guess the reason
What are the preventive methods do you take for rusting iron material
If n=3 ,mention the orbitals present in the shell and write maximum number of electrons in the shell
A person is unable to see distant objects , show the defect of vision of the person with the help of ray diagram
Iron displaces copper from CuSO4 solution and you will observe reddish brown copper deposit after some time. It is a displacement reaction. You can also explain this phenomenon in terms of oxidation and reduction. Fe which has an oxidation number of 0 gets oxidized to +2 state by forming FeSO4, while copper with an oxidation state of +2 in CuSO4 gets reduced to Cu with an oxidation state of 0. So, basically it's a redox reaction as well.
This can be explained using electrochemical series. Fe has less negative reduction potential (ability to get reduced is less, it's non-spontaneous) while copper has a positive reduction potential (its ability to get reduced is higher than iron, it's spontaneous). This is the main reason why Fe displaces Cu from copper sulphate solution. If you add copper to iron sulphate solution, no reaction is observed because Cu has higher reduction potential and hence it stays as Cu instead of displacing iron and getting oxidized to Cu2+.
2.
How to Prevent Corrosion Metal Type One simple way to prevent corrosion is to use a corrosion resistant metal such as aluminum or stainless steel. Depending on the application, these metals can be used to reduce the need for additional corrosion protection.
Protective Coatings The application of a paint coating is a cost-effective way of preventing corrosion. Paint coatings act as a barrier to prevent the transfer of electrochemical charge from the corrosive solution to the metal underneath.
Another possibility is applying a powder coating. In this process, a dry powder is applied to the clean metal surface. The metal is then heated which fuses the powder into a smooth unbroken film. A number of different powder compositions can be used, including acrylic, polyester, epoxy, nylon, and urethane.
Environmental Measures Corrosion is caused by a chemical reaction between the metal and gases in the surrounding environment. By taking measures to control the environment, these unwanted reactions can be minimized. This can be as simple as reducing exposure to rain or seawater, or more complex measures, such as controlling the amounts of sulfur, chlorine, or oxygen in the surrounding environment. An example of this would be would be treating the water in water boilers with softeners to adjust hardness, alkalinity, or oxygen content.
Sacrificial Coatings Sacrificial coating involves coating the metal with an additional metal type that is more likely to oxidize; hence the term “sacrificial coating.”
Dear student,
You are not supposed to ask multiple questions at a time.Please close the question and ask them as separate questions.Anyway I've solved 2 questions for you
Iron displaces copper from CuSO4 solution and you will observe reddish brown copper deposit after some time. It is a displacement reaction. You can also explain this phenomenon in terms of oxidation and reduction. Fe which has an oxidation number of 0 gets oxidized to +2 state by forming FeSO4, while copper with an oxidation state of +2 in CuSO4 gets reduced to Cu with an oxidation state of 0. So, basically it's a redox reaction as well.
This can be explained using electrochemical series. Fe has less negative reduction potential (ability to get reduced is less, it's non-spontaneous) while copper has a positive reduction potential (its ability to get reduced is higher than iron, it's spontaneous). This is the main reason why Fe displaces Cu from copper sulphate solution. If you add copper to iron sulphate solution, no reaction is observed because Cu has higher reduction potential and hence it stays as Cu instead of displacing iron and getting oxidized to Cu2+.
2.
How to Prevent Corrosion Metal TypeOne simple way to prevent corrosion is to use a corrosion resistant metal such as aluminum or stainless steel. Depending on the application, these metals can be used to reduce the need for additional corrosion protection.
Protective CoatingsThe application of a paint coating is a cost-effective way of preventing corrosion. Paint coatings act as a barrier to prevent the transfer of electrochemical charge from the corrosive solution to the metal underneath.
Another possibility is applying a powder coating. In this process, a dry powder is applied to the clean metal surface. The metal is then heated which fuses the powder into a smooth unbroken film. A number of different powder compositions can be used, including acrylic, polyester, epoxy, nylon, and urethane.
Environmental MeasuresCorrosion is caused by a chemical reaction between the metal and gases in the surrounding environment. By taking measures to control the environment, these unwanted reactions can be minimized. This can be as simple as reducing exposure to rain or seawater, or more complex measures, such as controlling the amounts of sulfur, chlorine, or oxygen in the surrounding environment. An example of this would be would be treating the water in water boilers with softeners to adjust hardness, alkalinity, or oxygen content.
Sacrificial CoatingsSacrificial coating involves coating the metal with an additional metal type that is more likely to oxidize; hence the term “sacrificial coating.”
Dear student,
You are not supposed to ask multiple questions at a time.Please close the question and ask them as separate questions.Anyway I've solved 2 questions for you
