Question

Consider the galvanic cell described by (n and m are metals): n(s)|N₂ (aq)||m (aq)|m(s) if eocathode = 0.258 v and eoanode = 1.068 v, and [N₂ (aq)] = 0.718 m and [m (aq)] = 0.254 m, what is ecell, using the nernst equation? ____ v

Answer 1

The cell potential for the galvanic cell can be calculated using the Nernst equation, which accounts for standard electrode potentials and reactant concentrations. Without the number of electrons transferred (n) and the reaction quotient (Q), we cannot provide a numerical answer, only the formula and steps needed for calculation.

Step-by-step explanation:

To calculate the cell potential (Ecell) for the given galvanic cell, we can use the Nernst equation, which will incorporate the standard electrode potentials and the concentrations of the reactants. The standard cell potential (E°cell) is found by subtracting the standard anode potential from the standard cathode potential:

E°cell = E°cathode - E°anode

Substituting the given values:

E°cell = 0.258 V - 1.068 V = -0.810 V

Now, applying the Nernst equation:

Ecell = E°cell - (0.0592V/n) · log Q

Where:
Q is the reaction quotient, n is the number of moles of electrons transferred in the balanced half-reactions, and Ecell is the cell potential at non-standard conditions.

However, since we do not have the values for n and Q (as the full half-reactions were not provided), we are unable to calculate the exact value of Ecell. Thus, we can only provide the formula and steps to calculate it but not the numerical answer.