Question

Consider the galvanic cell described by (n and m are metals): n(s)|N₂ (aq)||m (aq)|m(s). If eocathode = 0.074 V and eoanode = 1.497 V, and [N₂ (aq)] = 0.952 M and [m (aq)] = 0.484 M, what is the value of ecell using the Nernst equation?

Answer 1

The voltage of the galvanic cell is determined by first calculating the standard cell potential with the formula E°cell = Ecathode - Eanode, then using the Nernst equation. However, to complete the calculation, the number of electrons transferred (n) and the reaction quotient (Q) are also required.

Step-by-step explanation:

To calculate the voltage of the galvanic cell described by n(s)|N₂ (aq)||m (aq)|m(s) with the given standard electrode potentials and ion concentrations, we will use the Nernst equation. First, we determine the standard cell potential (E°cell) using the formula:

E°cell = Ecathode - Eanode

So, E°cell = 0.074 V - 1.497 V = -1.423 V.

Next, we use the Nernst equation:

Ecell = E°cell - (0.0592/n) log Q

However, we do not have the number of electrons transferred in the reaction (n) and the reaction quotient (Q). Generally, for full calculation, these values are needed. Assuming 'n' is known and Q = [product concentrations]/[reactant concentrations], we would then insert the appropriate values into the Nernst equation to find Ecell.