Hydrazene can be used in fuel cell
N2H4(aq)+o2(g)->N2(g)+2H2O(l)
IfΔG°for this reaction is -600kj what will be the E°for the cell?
To determine the standard cell potential (E°) for the given reaction, we can use the relationship between ΔG° and E°, which is given by the equation:
ΔG° = -nFE°
Where:
ΔG° is the standard Gibbs free energy change for the reaction,
n is the number of moles of electrons transferred in the balanced equation,
F is the Faraday constant (96,485 C/mol),
E° is the standard cell potential.
In the given reaction, the balanced equation shows that 2 moles of electrons are transferred. Therefore, n = 2 in this case.
We are given that ΔG° = -600 kJ. However, ΔG° is typically expressed in kilojoules per mole (kJ/mol), and we need to convert it to joules per mole (J/mol) to match the units of the Faraday constant.
1 kJ = 1000 J, so -600 kJ = -600,000 J.
Now, let's calculate E° using the equation:
ΔG° = -nFE°
-600,000 J/mol = -2(96,485 C/mol) x E°
Simplifying further:
-600,000 J/mol = -192,970 C x E°
Dividing both sides by -192,970 C, we get:
E° = -600,000 J/mol / -192,970 C
Evaluating the right side of the equation,
E° ≈ 3.11 V
Therefore, the standard cell potential (E°) for the given reaction is approximately 3.11 V.