Calculate for the Electrochemical Cell Below,
Ag(s)| AgCl(s)| Cl^-(aq,1 $\to$

Calculate for the electrochemical cell below,
Ag(s) | AgCl(s) | Cl^-(aq,1.0 M) || Cu²⁺(aq,1.0 M) | Cu(s)
Given the following standard reduction potentials.

Cu²⁺(aq) + 2 e^- $\to$ Cu(s) $~~~~~~~~$$~~~~~~~~$ E ^$\circ$ = +0.337 V
AgCl(s) + e^- $\to$ Ag(s) + Cl^-(aq) $~~~~~~~~$ E ^$\circ$ = +0.222 V

A) -0.115 V
B) -0.107 V
C) +0.115 V
D) +0.452 V
E) +0.559 V