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.
Predict the major organic product(s) of the following reactions. Indicate which of the following mechanisms is in operation: SN1, SN2, E1, or E2.
(c)
(4pts)
Mechanism:
heat
(E1)
CH3OH
+
1.5pts each
_E1 _ (1pt)
Br
CH3OH
(d)
(4pts)
Mechanism:
SN1
(1pt)
(e)
(3pts)
1111 I
H
10
Ill!!
H
LDA
THF (solvent)
Mechanism: E2
(1pt)
NC
(f)
Bri!!!!!
CH3
NaCN
(3pts)
acetone
Mechanism: SN2
(1pt)
(SN1)
-OCH3
OCH3
1.5pts each
2pts for either product
1pt if incorrect
stereochemistry
H
Br
(g)
“,、
(3pts)
H
CH3OH
+21
Mechanism:
SN2
(1pt)
H
CH3
2pts
1pt if incorrect
stereochemistry
H
2pts
1pt if incorrect
stereochemistry
A mixture of butyl acrylate and 4'-chloropropiophenone has been taken for proton NMR analysis. Based on this proton NMR, determine the relative percentage of each compound in the mixture
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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