Using the Following Data, Determine the Standard Cell Potential $$E _ { \text { cell} } ^ { \circ }$$

Using the following data, determine the standard cell potential $$E _ { \text { cell} } ^ { \circ }$$ for the electrochemical cell constructed using the following reaction, where zinc is the anode and lead is the cathode. $\mathrm{Zn}(s) +\mathrm{Pb}^{2+}(a q) \rightarrow \mathrm{Zn}^{2+}(a q) +\mathrm{Pb}(s)$
$\begin{array}{lll}\text { Potential } & \text { Half-reaction } & \text { Standard Reduction } \\& & \\& \mathrm{Zn}^{2+}(a q) +2 \mathrm{e}^{-} \rightarrow \mathrm{Zn}(s) & -0.763 \\& \mathrm{Ph}^{2+}(a a) +2 \mathrm{e}^{-} \rightarrow \mathrm{Ph}(s) & -0126\end{array}$

A) +0.637 V
B) -0.637 V
C) +1.274 V
D) -0.889 V
E) +0.889 V