How do the ions transfer between solutions in an electrochemical cell?

In a galvanic cell,the electrons flow from:

Using the standard electrode potentials given in Table $3.1$ of the $NCERT$ textbook,predict if the reaction between the following is feasible:
$(i)$ $Fe^{3+}_{(aq)}$ and $I^{-}_{(aq)}$
$(ii)$ $Ag^{+}_{(aq)}$ and $Cu_{(s)}$
$(iii)$ $Fe^{3+}_{(aq)}$ and $Br^{-}_{(aq)}$
$(iv)$ $Ag_{(s)}$ and $Fe^{3+}_{(aq)}$
$(v)$ $Br_{2(aq)}$ and $Fe^{2+}_{(aq)}$

Assertion : For the Daniel cell,$Zn|Zn^{2+} || Cu^{2+}|Cu$ with $E_{cell} = 1.1 \ V$,the application of an opposite potential greater than $1.1 \ V$ results in the flow of electrons from cathode to anode.
Reason : $Zn$ is deposited at the anode,and $Cu$ is deposited at the cathode.

The position of some metals in the electrochemical series in decreasing electropositive character is given as $Mg > Al > Zn > Cu > Ag$. What will happen if a copper spoon is used to stir a solution of aluminium nitrate?

Which of the following statements about a galvanic cell is incorrect?