The spontaneous reaction $\mathrm{Zn}(\mathrm{s})+2\mathrm{Fe}{}^{3+}(\mathrm{aq})\to \mathrm{Zn}{}^{2+}(\mathrm{aq})+2\mathrm{Fe}{}^{2+}(\mathrm{aq})$ is to be run in a galvanic cell. The correct cell notation is

Zn is oxidised, so $\mathrm{Zn}|\mathrm{Zn}{}^{2+}$ is the anode and is written on the left. The cathode half reaction $\mathrm{Fe}{}^{3+}+\mathrm{e}{}^{-}\to \mathrm{Fe}{}^{2+}$ has both species in solution, so an inert Pt electrode is needed and the two ions are separated by a comma, not a vertical line. Option B has no electrode, option C is reversed (would have negative EMF), option D reduces $\mathrm{Fe}{}^{2+}$ to Fe, which is a different reaction.