We're given the following galvanic cell:

**N( s) | N^{2+}(aq) || M^{+}(aq) | M(s)**

When writing a cell notation, we use the following format – “*as easy as ABC*”

**L**ose **G**ain**E**lectron **E**lectrons**O**xidation **R**eduction

• lose electrons → oxidation → anode

• gain electrons → reduction → cathode

Consider the galvanic cell described by (N and M are metals):

N(*s*) | N^{2+}(*aq*) || M^{+}(*aq*) | M(*s*)

If *E*°_{cathode} = 0.182 V and *E*°_{anode} = 1.411 V, and [N^{2+}(aq)] = 0.931 M and [M^{+}(aq)] = 0.655 M, what is *E*_{cell}, using the Nernst equation? ____ V

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