Respuesta :
The standard Gibbs free energy for the given redox reaction is -106kJ/mol.
What is the standard Gibbs free energy?
The standard Gibbs free energy (ΔG°) is a thermodynamic potential that can be used to calculate the maximum reversible work that may be performed by a thermodynamic system under standard conditions.
To find the Gibbs free energy, first we have to know about the redox reaction,
10 Cl⁻(aq) + 2 MnO₄⁻(aq) + 16 H⁺(aq) ⇒ 5 Cl₂(g) + 2 Mn²⁺(aq) + 8 H₂O(l)
As we have to analyze the standard reduction potentials (E°red).
Cathode: 2 MnO₄⁻ + 16 H⁺ + 10 e⁻ ⇒ 2 Mn²⁺ + 8 H₂O
E°red = 1.51 V
Anode: 10 Cl⁻ ⇒ 5 Cl₂ + 10 e⁻
E°red = 1.40 V
Then, the potential difference between the cathode and anode is called the standard cell potential.
E°cell = E°red, cathode - E°red, anode
= 1.51 V - 1.40 V
= 0.11 V
The standard cell potential is 0.11 V.
The Gibbs free energy can be calculated as,
ΔG° = - n × F × E°cell
ΔG° = - 10 mol × (96,485 J/V.mol) × 0.11 V × (1 kJ/1000 J)
= -106 kJ/mol
where,
n - moles of electrons exchanged.
F -Faraday's constant.
The standard Gibbs free energy for the given redox reaction is -106kJ/mol.
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