The equilibrium constant for the reaction
2Hg(l) + 2Cl^-(aq) + Ni²⁺(aq) $\rightarrow$ Ni(s) + Hg₂Cl₂(s)
Is 5.6 * 10^-²⁰ at 25^$\omicron$C.Calculate the value of E^$\omicron$for a cell utilizing this reaction.

Question

The equilibrium constant for the reaction
2Hg(l) + 2Cl^-(aq) + Ni²⁺(aq)

\rightarrow

Ni(s) + Hg₂Cl₂(s)
Is 5.6 * 10^-²⁰ at 25^$\omicron$C.Calculate the value of E^$\omicron$for a cell utilizing this reaction.

Quizplus · Accepted Answer

The equilibrium constant (K) is related to the standard cell potential (E°) by the Nernst equation: E° = (RT/nF)lnK. At 25°C, this simplifies to E° = (0.0592/n)logK. For this reaction, n = 2. Plugging in the values, E° = (0.0592/2)log(5.6 * 10^-20) = -0.57 V.

The Equilibrium Constant for the Reaction 2Hg(l)+ 2Cl-(aq)+ Ni2+(aq) →\rightarrow→ Ni(s)+ Hg2Cl2(s) Is 5

The Equilibrium Constant for the Reaction
2Hg(l)+ 2Cl^-(aq)+ Ni²⁺(aq) $\rightarrow$ Ni(s)+ Hg₂Cl₂(s)
Is 5