From the relation between E ∘ , Δ G ∘ and K, this is to be shown that the value of Δ G ∘ is negative and K > 1 for the reaction with a positive E ∘ value. Concept introduction: The substances that have a higher reduction potential will undergo reduction at the cathode while the substances that have a lower reduction potential will undergo oxidation at the anode. The expression to calculate the equilibrium constant is shown below: Δ G cell o = − RT ln K Here, R is Universal gas constant, T is temperature and K is equilibrium constant. The expression to calculate the standard Gibbs free energy of the cell is shown below: Δ G cell o = − nFE cell o Here, n is the number of electrons transferred, F is Faraday’s constant and E cell o is standard electrode potential of the cell.
From the relation between E ∘ , Δ G ∘ and K, this is to be shown that the value of Δ G ∘ is negative and K > 1 for the reaction with a positive E ∘ value. Concept introduction: The substances that have a higher reduction potential will undergo reduction at the cathode while the substances that have a lower reduction potential will undergo oxidation at the anode. The expression to calculate the equilibrium constant is shown below: Δ G cell o = − RT ln K Here, R is Universal gas constant, T is temperature and K is equilibrium constant. The expression to calculate the standard Gibbs free energy of the cell is shown below: Δ G cell o = − nFE cell o Here, n is the number of electrons transferred, F is Faraday’s constant and E cell o is standard electrode potential of the cell.
Solution Summary: The author analyzes the relation between Ecirc & Delta. The expression to calculate the standard Gibbs free energy of the cell is shown below.
From the relation between E∘, ΔG∘ and K, this is to be shown that the value of ΔG∘ is negative and K>1 for the reaction with a positive E∘ value.
Concept introduction:
The substances that have a higher reduction potential will undergo reduction at the cathode while the substances that have a lower reduction potential will undergo oxidation at the anode.
The expression to calculate the equilibrium constant is shown below:
ΔGcello=−RTlnK
Here, R is Universal gas constant, T is temperature and K is equilibrium constant.
The expression to calculate the standard Gibbs free energy of the cell is shown below:
ΔGcello=−nFEcello
Here, n is the number of electrons transferred, F is Faraday’s constant and Ecello is standard electrode potential of the cell.
So I need help with understanding how to solve these types of problems. I'm very confused on how to do them and what it is exactly, bonds and so forth that I'm drawing. Can you please help me with this and thank you very much!
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Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell