Question

Grey colored metal ‘X’ is used in making dry cell. It is also used for coating iron metal to prevent it from rusting .When granules of ‘X’ are added to pale green solution of compound of the most corrosive metal ‘Y’, the color of the solution gets faded and metal ‘Y’ is formed. Identify ’X’ and ‘Y’. Write the chemical equation of the reaction involved. When we add pure silver coin to this pale green solution of a compound of corrosive metal Y, explain what will happen?

Answer 1

Explanation:

Given -

• Grey coloured metal X is used in making dry cell.
• It is also used for coating iron and metal to prevent it from rusting.
• When granules of X are added to pale green solution of compound of the most corrosive metal Y, the colour of the solution faded and metal Y is formed.

To Find -

1. Identify X and Y
2. Write the chemical equation of the reaction involved.
3. When we add pure silver coin to this pale green solution of a compound of corrosive metal Y, explain what will happen?

Solution -

As we know that -

• Zinc is used in making dry cell and coating of iron and it is grey in colour.

So,

Metal X is Zinc (Zn).

When Zinc is added to copper sulphate (CuSO4) then Zinc sulphate (ZnSO4) and Copper (Cu) is produced.

Chemical equation -

Zn + CuSO4 → ZnSO4 + Cu

When we add silver coin to copper sulphate solution then Silver doesn't displace Copper from copper sulphate because silver is less reactive than copper.

Hence,

Metal X is Zinc (Zn).

Metal Y is Copper (Cu).