Question

Determine the equilibrium constant at 255 K for the following reaction under acidic conditions 4H+(aq) + MnO, (s) +2Fe2+ (aq)-> Mn2+ (aq) +2Fe3+ (aq) + 2H,0? The two half-reactions are: MnO2(s) +4H+(aq) + 2e-? Mn2+(aq) + 2H20(1) E?-1.23 V Fe3-(aq) + e-? Fe2 + (ag) E -0.770 V

Answer 1

To determine the equilibrium constant at 255 K for the given reaction under acidic conditions, use the Nernst equation and the half-reactions provided to write the balanced equation. Then, calculate the equilibrium constant using the concentrations of the species.

Step-by-step explanation:

The equilibrium constant for a reaction under acidic conditions can be determined using the Nernst equation. In this case, we can use the half-reactions given to write the balanced equation for the overall reaction:

4H+(aq) + MnO2(s) + 2Fe2+(aq) -> Mn2+(aq) + 2Fe3+(aq) + 2H2O

The equilibrium constant (K) at 255 K can be calculated using the concentrations of the species involved and plugging them into the equation:

K = [Mn2+][Fe3+]2 / [H+]4