A half-reaction and its reduction potential is given. By using these values, the equilibrium constant K for the given equilibrium reaction is to be calculated. Concept introduction: The relationship between reduction potential and standard reduction potential value and activities of species present in an electrochemical cell at a given temperature is given by the Nernst equation. The value of E cell is calculated using Nernst formula, E = E ° − ( R T n F ) ln ( Q ) At room temperature the above equation is specifies as, E = E ° − ( 0.0591 n ) log ( Q ) This relation is further used to determine the relation between Δ G ° and K , Δ G ° and E ° cell . The value of equilibrium constant is used to predict the extent of the reaction. To determine: The value of equilibrium constant K for the given equilibrium reaction.
A half-reaction and its reduction potential is given. By using these values, the equilibrium constant K for the given equilibrium reaction is to be calculated. Concept introduction: The relationship between reduction potential and standard reduction potential value and activities of species present in an electrochemical cell at a given temperature is given by the Nernst equation. The value of E cell is calculated using Nernst formula, E = E ° − ( R T n F ) ln ( Q ) At room temperature the above equation is specifies as, E = E ° − ( 0.0591 n ) log ( Q ) This relation is further used to determine the relation between Δ G ° and K , Δ G ° and E ° cell . The value of equilibrium constant is used to predict the extent of the reaction. To determine: The value of equilibrium constant K for the given equilibrium reaction.
Solution Summary: The author explains how the Nernst equation calculates the equilibrium constant K for the given half-cell reaction.
Definition Definition Chemical reactions involving both oxidation and reduction processes. During a redox reaction, electron transfer takes place in such a way that one chemical compound gets reduced and the other gets oxidized.
Chapter 17, Problem 90E
Interpretation Introduction
Interpretation:
A half-reaction and its reduction potential is given. By using these values, the equilibrium constant K for the given equilibrium reaction is to be calculated.
Concept introduction:
The relationship between reduction potential and standard reduction potential value and activities of species present in an electrochemical cell at a given temperature is given by the Nernst equation.
The value of Ecell is calculated using Nernst formula,
E=E°−(RTnF)ln(Q)
At room temperature the above equation is specifies as,
E=E°−(0.0591n)log(Q)
This relation is further used to determine the relation between ΔG° and K, ΔG° and E°cell. The value of equilibrium constant is used to predict the extent of the reaction.
To determine: The value of equilibrium constant K for the given equilibrium reaction.
4. Provide a clear arrow-pushing mechanism for each of the following reactions. Do not skip proton
transfers, do not combine steps, and make sure your arrows are clear enough to be interpreted
without ambiguity.
a.
2.
1. LDA
3. H3O+
HO
b.
H3C CH3
H3O+
✓ H
OH
2. Provide reagents/conditions to accomplish the following syntheses. More than one step is
required in some cases.
a.
CH3
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