Question #44724

To model the thermodynamic effect of osmotic stress on the cathodic half-reaction of iron corrosion, a concentration cell is constructed using two identical Platinum electrodes. Both compartments are continuously purged with $\ce{O2(g)}$ at $1 \text{ bar}$ and maintained at $\text{pH} = 10.0$ at $298 \text{ K}$.

Compartment A contains pure water. Compartment B contains a hypertonic aqueous solution of a non-volatile, non-electrolyte solute, generating an osmotic pressure of $\Pi = 21.44 \text{ MPa}$.

Assuming the activity coefficients of the ions are unaffected by the solute, what is the magnitude of the cell potential ($E_{\text{cell}}$) generated, and which compartment acts as the anode?

(Given: Molar volume of liquid water $V_m = 18.0 \text{ cm}^3 \text{ mol}^{-1}$, Faraday constant $F = 96500 \text{ C mol}^{-1}$. Assume ideal behavior for the gas.)