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 a nickel metal electrode immersed in a solution with a given concentration and is separated by a porous disk from an aluminum metal electrode.
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 a nickel metal electrode immersed in a solution with a given concentration and is separated by a porous disk from an aluminum metal electrode.
Solution Summary: The author describes an electrochemical cell with a standard hydrogen electrode and copper metal electrode as the reference electrode for the calculation of standard reduction potential of other electrodes.
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 18, Problem 80E
(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 a nickel metal electrode immersed in a solution with a given concentration and is separated by a porous disk from an aluminum metal electrode.
(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
Al3+ at the given measured potential.
Vnk the elements or compounds in the table below in decreasing order of their boiling points. That is, choose 1 next to the substance with the highest bolling
point, choose 2 next to the substance with the next highest boiling point, and so on.
substance
C
D
chemical symbol,
chemical formula
or Lewis structure.
CH,-N-CH,
CH,
H
H 10: H
C-C-H
H H H
Cale
H 10:
H-C-C-N-CH,
Bri
CH,
boiling point
(C)
Сен
(C) B
(Choose
Please help me find the 1/Time, Log [I^-] Log [S2O8^2-], Log(time) on the data table. With calculation steps. And the average for runs 1a-1b. Please help me thanks in advance. Will up vote!
Q1: Answer the questions for the reaction below:
..!! Br
OH
a) Predict the product(s) of the reaction.
b) Is the substrate optically active? Are the product(s) optically active as a mix?
c) Draw the curved arrow mechanism for the reaction.
d) What happens to the SN1 reaction rate in each of these instances:
1. Change the substrate to
Br
"CI
2. Change the substrate to
3. Change the solvent from 100% CH3CH2OH to 10% CH3CH2OH + 90% DMF
4. Increase the substrate concentration by 3-fold.
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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