The standard cell potential, E°cell, for a reaction in which two electrons are transferred between the reactants is +1.33 V. Cal

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The standard cell potential, E°cell, for a reaction in which two electrons are transferred between the reactants is +1.33 V. Cal

culate 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

Chemistry

1 answer:

Alinara [238K] · Answer 1 · 2022-05-14T12:59:56+03:00

Answer:

ΔG° = 2.57 × 10² kJ

The reaction is spontaneous.

Explanation:

<em>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.</em>

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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.