The electrochemical cell shown below is a concentration cell. M | M²⁺ (saturated solution of a sparingly soluble salt, MX₂) || M²⁺ (0.001 mol dm^–3) | M The emf of the cell depends on the difference in concentrations of M²⁺ ions at the two electrodes. The emf of the cell at 298 K is 0.059 V.

The value of ∆G (kJ mol^–1) for the given cell is (take 1F = 96500 C mol^–1)

Consider the following cell reaction:
2Fe(s) + O₂(g) + 4H⁺(aq) $$\to$$ 2Fe²⁺ (aq) + 2H₂O (l); E^o = 1.67 V
At [Fe²⁺] = 10^-3 M, P(O₂) = 0.1 atm and pH = 3, the cell potential at 25^oC is

The concentration of potassium ions inside a biological cell is at least twenty times higher than the outside. The resulting potential difference across the cell is important in several processes such as transmission of nerve impulses and maintaining the ion balance. A simple model for such a concentration cell involving a metal M is :
M(s) | M⁺ (aq ; 0.05 molar) || M⁺ (aq ; 1 molar) | M(s)
For the above electrolytic cell the magnitude of the cell potential | E_cell | = 70 mV.

For the above cell :

The concentration of potassium ions inside a biological cell is at least twenty times higher than the outside. The resulting potential difference across the cell is important in several processes such as transmission of nerve impulses and maintaining the ion balance. A simple model for such a concentration cell involving a metal M is :
M(s) | M⁺ (aq ; 0.05 molar) || M⁺ (aq ; 1 molar) | M(s)
For the above electrolytic cell the magnitude of the cell potential | E_cell | = 70 mV.

If the 0.05 molar solution of M⁺ is replaced by a 0.0025 molar M⁺ solution, then the magnitude of the cell potential would be :