The concentration of Cu 2+ in CuSO 4 solution needs to be determined if the measured cell potential at 25°C is 0.67 V and the galvanic cell has an iron electrode in contact with 0.10 M FeSO 4 and a copper electrode in contact with CuSO 4 solution. Concept introduction: In the electrochemical cell, the reactions at cathode and anode occur due to the difference in their reduction electrode potential value. The EMF of the cell can be calculated with the help of electrode reduction potential values. The reaction at each electrode is called as half-reaction and the combination of both half-reactions gives the cell reaction of given electrochemical cell. The standard cell potential for an electrochemical cell can be calculated as: E cell ° = E cathode ° - E anode ° E cell ° = E reduction ° - E oxidation ° The potential of a cell can be calculated with the help of the Nernst equation that can be shown as: E° = E° cell - 0 .0592 V n log Q n = number of electrons Q = reaction quotient
The concentration of Cu 2+ in CuSO 4 solution needs to be determined if the measured cell potential at 25°C is 0.67 V and the galvanic cell has an iron electrode in contact with 0.10 M FeSO 4 and a copper electrode in contact with CuSO 4 solution. Concept introduction: In the electrochemical cell, the reactions at cathode and anode occur due to the difference in their reduction electrode potential value. The EMF of the cell can be calculated with the help of electrode reduction potential values. The reaction at each electrode is called as half-reaction and the combination of both half-reactions gives the cell reaction of given electrochemical cell. The standard cell potential for an electrochemical cell can be calculated as: E cell ° = E cathode ° - E anode ° E cell ° = E reduction ° - E oxidation ° The potential of a cell can be calculated with the help of the Nernst equation that can be shown as: E° = E° cell - 0 .0592 V n log Q n = number of electrons Q = reaction quotient
Solution Summary: The author explains the Nernst equation for calculating the cell potential of an electrochemical cell. The reaction at each electrode is called half-reaction.
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 19, Problem 19.97SP
Interpretation Introduction
Interpretation:
The concentration of Cu2+ in CuSO4 solution needs to be determined if the measured cell potential at 25°C is 0.67 V and the galvanic cell has an iron electrode in contact with 0.10 M FeSO4 and a copper electrode in contact with CuSO4 solution.
Concept introduction:
In the electrochemical cell, the reactions at cathode and anode occur due to the difference in their reduction electrode potential value. The EMF of the cell can be calculated with the help of electrode reduction potential values. The reaction at each electrode is called as half-reaction and the combination of both half-reactions gives the cell reaction of given electrochemical cell. The standard cell potential for an electrochemical cell can be calculated as:
→
Acetyl-CoA + 3NAD+ + 1FAD + 1ADP 2CO2 + CoA + 3NADH + 1FADH2 + 1ATP
a. Which of the above are the reactants?
b. Which of the above are the products?
c. Which reactant is the electron donor?
d. Which reactants are the electron acceptors?
e. Which of the products are now reduced?
f. Which product is now oxidized?
g. Which process was used to produce the ATP?
h. Where was the energy initially in this chemical reaction and where is it now that it is
finished?
i. Where was the carbon initially in this chemical reaction and where is it now that it is
finished?
j. Where were the electrons initially in this chemical reaction and where is it now that it is
finished?
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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