Consider an Electrochemical Cell with a Zinc Electrode Immersed in 1.0

Consider an electrochemical cell with a zinc electrode immersed in 1.0 M Zn²⁺ and a silver electrode immersed in 1.0 M Ag⁺. Zn²⁺ + 2e^- $\to$ Zn $\varepsilon$ ^$\circ$ = -0.755 V
Ag⁺ + e^- $\to$ Ag $\varepsilon$ ^$\circ$ = 0.800 V
Calculate $\varepsilon$ ^$\circ$ for this cell.

A) 0.045 V
B) -0.045 V
C) 1.555 V
D) -1.555 V
E) none of these