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.

dG = -nFEo