Consider an Electrochemical Cell Consisting of an Fe(s) Electrode, Fe(NO₃)₂ $\rarr$

Consider an electrochemical cell consisting of an Fe(s) electrode, Fe(NO₃) ₂ electrolyte connected through a salt bridge to a Ag wire coated in AgCl(s) immersed in an aqueous KCl solution. Is the standard cell and balanced galvanic cell reaction:(If needed, refer to Table 17-1 in the text )

A) 0.259 V, Fe(s) + 3AgCl(s) $\rarr$ Fe³⁺(aq) + 3Ag(s) + 3Cl^-(aq)
B) 0.669 V, Fe(s) + 2AgCl(s) $\rarr$ Fe²⁺(aq) + 2Ag(s) + 2Cl^-(aq)
C) -0.669 V, Fe(s) + 2AgCl(s) $\rarr$ Fe²⁺(aq) + 3Ag(s) + 3Cl^-(aq)
D) -0.225 V, Fe(s) + 2AgCl(s) $\rarr$ Fe²⁺(aq) + 2Ag(s) + 2Cl^-(aq)
E) 0.669 V, Fe(s) + AgCl(s) $\rarr$ Fe²⁺(aq) + Ag(s) + Cl^-(aq)