Calculate Keq for 2 moles of electron(s) in each half-reaction and a standard potential of 0.55 V.
To calculate the equilibrium constant (Keq) for a given half-reaction, you need to know the standard potential (E°) and the number of moles of electrons involved.
The Nernst equation relates the standard potential to the equilibrium constant:
E = E° - (RT / nF) * ln(Keq)
Where:
- E is the cell potential under non-standard conditions
- E° is the standard cell potential
- R is the gas constant (8.314 J/(mol·K))
- T is the temperature in Kelvin
- n is the number of moles of electrons transferred in the balanced half-reaction
- F is Faraday's constant (96485 C/mol)
In this case, the standard potential (E°) is given as 0.55 V, and the number of moles of electrons transferred (n) is 2.
Assuming the temperature is constant, we can calculate Keq using the Nernst equation:
Keq = exp((E° - E) * (nF / RT))
Since we're given the standard potential (E°) and the number of moles of electrons (n), we don't have enough information to calculate Keq without knowing the actual cell potential (E).