A large piece of zinc metal is placed in a copper (II) sulfate, $C u S O_{4}$ solution. The blue solution becomes colourless as copper metals fall to the bottom of the container. The resulting solution contains zinc sulfate, $Z n S O_{4}$ . Write a balanced chemical equation for the reaction.

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Solution

The balanced chemical reaction is
$Z n (s) + C u S O_{4} (a q) 🡪 C u (s) + Z n S O_{4} (a q) (z i n c) (c o p p e r s u l p h a t e) (c o p p e r) (z i n c s u l p h a t e)$
In this displacement reaction, the more reactive metal, zinc, displace the ions of the less reactive metal, copper, from its aqueous solution.
$Z n (s) + C u S O_{4} (a q) 🡪 C u (s) + Z n S O_{4} (a q)$

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Study the type of chemical reaction taking place when zine metal reacts with copper sulfate and complete the observation and conclusion.

Things needed: A beaker, zinc metal, copper sulfate solution.

Method:

Observation : (i) Colour changes from sky blue to ........

(ii) The reaction is ................. (exothermic or endothermic).

(iii) ........ metal precipitated as solid.

(iv) Type of reaction ...........

Conclusion: Chemical equation is $Zn + {CuSO}_{4} \to$

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