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What will occur if a block of copper metal is dropped into a beaker containing a solution of 1M ${ZnSO}_{4}$ ?

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The copper metal will dissolve and zinc metal will be deposited.

No reaction will occur.

The copper metal will dissolve with evolution of oxygen gas.

The copper metal will dissolve with evolution of hydrogen gas.

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detailed solution

Correct option is B

Zinc cannot be removed from ${ZnSO}_{4}$ by copper.
As a result, nothing will happen.

Notably, ${Zn}^{2 +} ∣ Zn$ has a lower standard reduction potential than ${Cu}^{2 +} ∣ Cu$ does.

Therefore, $Zn$ is a better reducer than $Cu$ . $Zn$ can therefore remove $Cu$ from copper sulphate solution.

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What will occur if a block of copper metal is dropped into a beaker containing a solution of 1M ZnSO4 ?

Unlock the full solution & master the concept.

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What will occur if a block of copper metal is dropped into a beaker containing a solution of 1M ${ZnSO}_{4}$ ?