The cell potential at 25°C for the following galvanic cell and the concentration of Cu 2+ when the cell potential drops to zero to maintain the concentration of Pb 2+ at 1.0 M should be determined: Pb (s) |Pb 2+ (1 .0 M) || Cu 2+ (1 .0 × 10 -4 M)|Cu (s) 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 the 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 cell potential at 25°C for the following galvanic cell and the concentration of Cu 2+ when the cell potential drops to zero to maintain the concentration of Pb 2+ at 1.0 M should be determined: Pb (s) |Pb 2+ (1 .0 M) || Cu 2+ (1 .0 × 10 -4 M)|Cu (s) 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 the 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 that the cell potential at 25°C for the following galvanic cell should be determined by the Nernst equation. The reaction at each electrode is called as 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 19.96SP
Interpretation Introduction
Interpretation:
The cell potential at 25°C for the following galvanic cell and the concentration of Cu2+ when the cell potential drops to zero to maintain the concentration of Pb2+ at 1.0 M should be determined:
Pb(s)|Pb2+(1.0 M) || Cu2+(1.0×10-4M)|Cu(s)
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:
1) Calculate the longest and shortest wavelengths in the Lyman and Paschen series.
2) Calculate the ionization energy of He* and L2+ ions in their ground states.
3) Calculate the kinetic energy of the electron emitted upon irradiation of a H-atom in ground state by a 50-nm radiation.
Calculate the ionization energy of He+ and Li²+ ions in their ground states.
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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