What will occur if a block of copper metal is dropped into a beaker containing a solution of 1M ${\mathrm{ZnSO}}_4$ ?

Zinc cannot be removed from ${\mathrm{ZnSO}}_4$ by copper.
As a result, nothing will happen.

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

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