# Problem: Consider the galvanic cell described by (N and M are metals): N(s)|N2+(aq) || M+(aq)|M(s) If E°cathode0 = 0.988 V and E°anode° = 1.606 V, and [N2+ (aq)] = 0.472 M and [M+(aq)) = 0.929 M, what is Ecell, using the Nernst equation? __V Provide your response to two digits after the decimal.

###### FREE Expert Solution

Calculate E°cell

$\overline{){\mathbf{E}}{{\mathbf{°}}}_{{\mathbf{cell}}}{\mathbf{=}}{\mathbf{E}}{{\mathbf{°}}}_{{\mathbf{cathode}}}{\mathbf{-}}{\mathbf{E}}{{\mathbf{°}}}_{{\mathbf{anode}}}}$

cell = 0.988 V – 1.606 V

cell = -0.618

Calculate for the initial cell potential using the initial concentrations of the species using the Nernst Equation.

Given:

E°cell = -0.618 V
n = 2 e-
[N2+] = 0.472 M
[M+] = 0.929 M

The reaction involved:

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

N(s)|N2+(aq) || M+(aq)|M(s)

If E°cathode0 = 0.988 V and E°anode° = 1.606 V, and [N2+ (aq)] = 0.472 M and [M+(aq)) = 0.929 M, what is Ecell, using the Nernst equation? __V

Provide your response to two digits after the decimal.