Silver wire is dipped in $0\mathrm{.}5M$ solution of silver ions and nickel electrode is dipped in $0\mathrm{.}2M$ solution of nickel ions.

The cell reaction is given as:

$Ni(s)+2A{g}^{+}(aq)N{i}^{2+}(aq)+2Ag(s)$

Note: Silver ions are undergoing reduction at cathode while nickel metal is undergoing oxidation at anode.

a$.$ What is the reaction quotient $(O)?($Hint$,$ plug in $N{i}^{2+}$ and $2A{g}^{+}$to the equations provided and use the concentrations given$)$

b$.$ Calculate the standard cell potential given, $E_{ox}^o=-0\mathrm{.}25V$ and $E_{\text{r}\text{e}\text{d}}^o=0\mathrm{.}7994V$

c$.$ How many electrons are involved in this reaction?

d$.$ Finally, what is the cell potential of this reaction $(E_{\text{c}\text{e}\text{l}\text{l}})?($Use the equations provided above$)($Double check your units!$)$