A redox reaction with E° = -2.25 V involving the transference of 6 moles of electrons has a ΔG° of 9.38 × 10⁵ J.
What is the standard Gibbs free energy?
The standard Gibbs free energy (ΔG°) is a thermodynamical function that indicates the spontaneity of a reaction.
A redox reaction, in which 6 moles of electrons are transferred (n = 6 mol), has a standard cell potential (E°) of -2.25 V.
Knowing that the Faraday's constant is F = 96,500 J/V.mol, we can calculate the standard Gibbs free energy using the following expression.
ΔG° = - n × F × E°
ΔG° = - 6 mol × (96,500 J/V.mol) × (-2.25 V) = 9.38 × 10⁵ J
A redox reaction with E° = -2.25 V involving the transference of 6 moles of electrons has a ΔG° of 9.38 × 10⁵ J.
Learn more about the standard Gibbs free energy here: https://brainly.com/question/9908454
