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

A
The copper metal will dissolve with evolution of oxygen gas
B
The copper metal will dissolve with evolution of hydrogen gas
C
No reaction will occur
D
The copper metal will dissolve and zinc metal will be deposited

Solution:

If a block of copper metal is dropped into a beaker containing a solution of $1 M {ZnSO}_{4}$ is no reaction will occur.

Zinc cannot be removed from ${ZnSO}_{4}$ by copper. As a result, nothing will happen.
Notably, ${Cu}^{2 +} ∣ Cu$ has a higher standard reduction potential than ${Zn}^{2 +} ∣ Zn$ .

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

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

Solution:

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