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A solution of CuSO4 was kept in an iron ...

 A solution of `CuSO_4` was kept in an iron pot. After 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. 

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We know that iron metal is more reactive than copper metal. So, when a solution of cppper sulphate `(CuSO_(4))` was kept in an iron pot, then iron being more reactive displaced copper of copper sulphate solution to form copper metal and iron (II) solution. the equation for this displacement reaction can be written as:
`underset("Copper (II) sulphate (Blue solution)")(CuSO_(4)(aq))+underset("Iron metal (From iron pot)")(Fe(s))tounderset("Iron (II) sulphate (Greenish solution)")(FeSO_(4)(aq))+underset("Copper metal")(Cu(s))`
Since the iron metal taking part in this displacement reaction is being taken from the iron pot, so holes are formed at those places in the iron pot from where iron metal has dissolved to form iron (II) sulphate.
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