Calculate ΔGo (in J) for 2 moles of electron(s) in each half-reaction and a standard potential of 0.44 V
To calculate ΔGo (standard Gibbs free energy change) for the given half-reaction, you need to use the equation:
ΔGo = -nFΔEo
Where:
- ΔGo is the standard Gibbs free energy change in joules (J)
- n is the number of moles of electrons transferred in the half-reaction
- F is the Faraday constant (96,485 C/mol)
- ΔEo is the standard potential (also known as the standard electrode potential) in volts (V)
Given:
n = 2 moles of electrons
ΔEo = 0.44 V
Firstly, let's convert the number of moles of electrons (n) to coulombs (C). Since 1 mole of electrons is equal to the charge of 1 Faraday, we can calculate the total charge (Q) in coulombs:
Q = n × F
Q = 2 × 96,485 C
Now, substitute the values into the equation:
ΔGo = -nFΔEo
ΔGo = -(2 × 96,485 C) × 0.44 V
Simplify the equation:
ΔGo = -192,970 C × 0.44 V
Finally, calculate ΔGo:
ΔGo = -84,910.8 J
Therefore, the ΔGo for the given half-reaction is -84,910.8 J.