Question

Consider the galvanic cell described by (n and m are metals): n(s)|N₂ (aq)||m (aq)|m(s). If eocathode = 0.7 V and eoanode = 1.737 V, and [N₂ (aq)] = 0.496 M and [m (aq)] = 0.017 M, what is the value of ecell using the Nernst equation? Provide your response to two digits after the decimal.

Answer 1

Using the given standard electrode potentials and concentrations, the standard cell potential is calculated first, then the Nernst equation is applied with provided concentrations to find the cell potential under non-standard conditions.

Step-by-step explanation:

To calculate the cell potential (Ecell) using the Nernst equation, we need to know both the standard electrode potentials and the concentration of the species involved. We are given that E◦cathode = 0.7 V and E◦anode = 1.737 V, with concentrations [N2 (aq)] = 0.496 M and [m (aq)] = 0.017 M.

The standard cell potential (E◦cell) is calculated as:
E◦cell = E◦cathode - E◦anode

Using the information provided:
E◦cell = 0.7 V - 1.737 V = -1.037 V

Now, we apply the Nernst equation to account for the non-standard conditions:

Ecell = E◦cell - (0.0592/n) log Q
where Q is the reaction quotient, and n is the number of electrons transferred in the balanced overall reaction.

Without the balanced reaction, we cannot determine the value of n. However, assuming n is known, and using concentrations provided, we would use Q = [m (aq)] / [N2 (aq)] to find Ecell.