The standard cell potential, e°cell, for a reaction in which two electrons are transferred between the reactants is +1.33 v. calculate the standard free energy change, δg°, in kj for this reaction and determine if it is spontaneous or nonspontaneous at 25°c. view available hint(s) the standard cell potential, e°cell, for a reaction in which two electrons are transferred between the reactants is +1.33 v. calculate the standard free energy change, δg°, in kj for this reaction and determine if it is spontaneous or nonspontaneous at 25°c. −1.28 × 102 kj, spontaneous −2.57 × 102 kj, spontaneous −2.57 × 102 kj, nonspontaneous +2.57 × 102 kj, nonspontaneous

ΔG° = 2.57 × 10² kJ

The reaction is spontaneous.

Explanation:

The standard cell potential, E°cell, for a reaction in which two electrons are transferred between the reactants is +1.33 V. Calculate the standard free energy change, ΔG°, in kJ for this reaction and determine if it is spontaneous or nonspontaneous at 25°C.

We can calculate the standard Gibbs free energy (ΔG°) using the following expression.

ΔG° = -n × F × E°cell

where,

n: moles of electrons transferred

F: Faraday's constant

E°cell: standard cell potential

ΔG° = - (2 mol) × (96468 J/V . mol) × 1.33 V

ΔG° = -2.57 × 10⁵ J = 2.57 × 10² kJ

ΔG° < 0 means that the reaction is spontaneous.

the answer is 303.15 or 303

its first and third is your answer i did the qustion the fourth isnt right