a solution of copper sulphate was kept in a iron pot. after a few days, the pot developed some holes in it . How will you a ccount for this

Open in App

Solution

Iron is more reactive than copper and so placed above copper in the reactivity series. Hence, when a solution of copper sulphate is placed in an iron pot, the iron metal from the pot will displace copper metal from CuSO₄ solution, thereby forming ferrous sulphate and copper metal. The blue colour of copper metal will slowly fade away and copper metal will also be deposited. Following is the chemical equation for the reaction
Fe + CuSO₄ â†’ FeSO₄ + Cu
Hence, holes will be developed in iron pot due to displacement reaction taking place between iron metal and CuSO₄ solution.

Suggest Corrections

Similar questions

What will happen if you keep a solution of copper sulphate in an iron container for a few days? What is the reason for your observation

Q. Brain Nurtures
A solution of

C u S O_{4}

was kept in an iron pot. After a few days, the iron pot was found to have a number of holes in it. How were these holes formed?

Q. A solution of

C u S O_{4}

was kept in an iron pot. After few days the iron pot was found to have a number of holes in it. The balance equation of the reaction involve is:

Q. A solution of

{CuSO}_{4}

was kept in an iron pot. After a few days, the iron pot was found to have a number of holes in it. Explain the reason in terms of reactivity. Write the equation of the reaction involved.

A zinc plate was put into a solution of copper sulphate kept in a glass tumbler. It was found that a blue colour of the solution gets fader and fader with the passage of time . After a few days when zinc plate was taken out, a no. of holes were found .

(i) state the reason for the change in the plate

Join BYJU'S Learning Program