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 nickel electrode immersed in 0.39 M Ni²⁺. Zn²⁺ + 2e^- $\to$ Zn
$\varepsilon$ ° = -0.76 V
Ni²⁺ + 2e^- $\to$ Ni
$\varepsilon$ ° = -0.23 V
Calculate $\varepsilon$ for this cell.

A) 0.54 V
B) 0.52 V
C) 0.51 V
D) 0.53 V
E) 0.98 V