Calculate ΔGo (in J) for 2 moles of electron(s) in each half-reaction and a standard potential of 0.57 V.
To calculate ΔGo (standard Gibbs free energy change) for a half-reaction, you can use the equation:
ΔGo = -nFΔEo
Where:
- ΔGo is the standard Gibbs free energy change (in J)
- n is the number of moles of electrons exchanged
- F is Faraday's constant (96,485 C/mol)
- ΔEo is the standard cell potential (in V)
In the given problem, n (number of moles of electrons exchanged) is 2, and ΔEo (standard cell potential) is 0.57 V.
Plugging these values into the equation:
ΔGo = - (2 mol) * (96,485 C/mol) * (0.57 V)
Now, let's calculate this:
ΔGo = - 2 * 96,485 * 0.57
ΔGo = - 110,573.2 J
Therefore, the standard Gibbs free energy change (ΔGo) for the given half-reaction is approximately -110,573.2 J.