An electrochemical cell with a standard hydrogen electrode and a copper metal electrode is given. Various questions based on the given concentration of ions and cell potential are to be answered. Concept introduction: The standard reduction potential for hydrogen ion is zero, therefore the standard hydrogen electrode is chosen as the reference electrode for the calculation of standard reduction potential of other electrodes. 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 ) To determine: The potential of the cell at 25 ° C if the copper electrode is placed in a given concentration of solution.
An electrochemical cell with a standard hydrogen electrode and a copper metal electrode is given. Various questions based on the given concentration of ions and cell potential are to be answered. Concept introduction: The standard reduction potential for hydrogen ion is zero, therefore the standard hydrogen electrode is chosen as the reference electrode for the calculation of standard reduction potential of other electrodes. 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 ) To determine: The potential of the cell at 25 ° C if the copper electrode is placed in a given concentration of solution.
Definition Definition Study of chemical reactions that result in the production of electrical energy. Electrochemistry focuses particularly on how chemical energy is converted into electrical energy and vice-versa. This energy is used in various kinds of cells, batteries, and appliances. Most electrochemical reactions involve oxidation and reduction.
Chapter 17, Problem 79E
(a)
Interpretation Introduction
Interpretation:
An electrochemical cell with a standard hydrogen electrode and a copper metal electrode is given. Various questions based on the given concentration of ions and cell potential are to be answered.
Concept introduction:
The standard reduction potential for hydrogen ion is zero, therefore the standard hydrogen electrode is chosen as the reference electrode for the calculation of standard reduction potential of other electrodes.
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)
To determine: The potential of the cell at
25°C if the copper electrode is placed in a given concentration of solution.
(b)
Interpretation Introduction
Interpretation:
An electrochemical cell with a standard hydrogen electrode and a copper metal electrode is given. Various questions based on the given concentration of ions and cell potential are to be answered.
Concept introduction:
The standard reduction potential for hydrogen ion is zero, therefore the standard hydrogen electrode is chosen as the reference electrode for the calculation of standard reduction potential of other electrodes.
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)
To determine: The value of concentration of
Cu2+ at the given measured potential.
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Draw a free-radical mechanism for the following reaction, forming the major monobromination product:
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CH3
Br-Br
CH
H3
Draw all missing reactants and/or products in the appropriate boxes by placing atoms on the canvas and connecting them with bonds. Add charges where needed. Electron-
flow arrows should start on the electron(s) of an atom or a bond and should end on an atom, bond, or location where a new bond should be created. Include all free radicals by
right-clicking on an atom on the canvas and then using the Atom properties to select the monovalent radical.
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DE
[1]
H EXP.
CONT.
H.
Br-Br
H
FEB
12
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Chapter 17 Solutions
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