Exercise 3: The following reduction reactions are given:(a) O,+2H;O+4e = 40H(b) O,+4H*+4e = 2H;OShow that the single electrode potential for each reaction at 25°C has the samepotential dependence.

Answered: Image /qna-images/answer/a2e8943b-68c9-4c86-8f0e-c98bd7547587.jpg

Exercise 3: The following reduction reactions are given: (a) O,+2H;O+4e = 40H (b) O,+4H*+4e = 2H;O %3D Show that the single electrode potential for each reaction at 25°C has the same potential dependence.

Exercise 3: The following reduction reactions are given: (a) O,+2H;O+4e = 40H (b) O,+4H*+4e = 2H;O %3D Show that the single electrode potential for each reaction at 25°C has the same potential dependence.

General Chemistry - Standalone book (MindTap Course List)

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ISBN:9781305580343

Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

Publisher:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

Chapter19: Electrochemistry

Section19.7: Dependence Of Cell Potential On Concentration

Problem 19.14E: What is the nickel(II)-ion concentration in the voltaic cell Zn(s)Zn2+(1.00M)Ni2+(aq)Ni(s) if the...

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Exercise 3: The following reduction reactions are given:
(a) O,+2H;O+4e = 40H
(b) O,+4H*+4e = 2H;O
Show that the single electrode potential for each reaction at 25°C has the same
potential dependence.

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If you were to construct a wet cell and decided to replace the salt bridge with a piece of copper wire, would the cell produce a sustainable current? Explain your answer.
Learning Goal: To learn how to use the Nernst equation. The standard reduction potentials listed in any reference table are only valid at the common reference temperature of 25∘C and standard conditions of 1 MM for solutions and 1 atm for gases. To calculate the cell potential at nonstandard conditions, one uses the Nernst equation, E=E∘−(2.303RT/nF) log10Q where E is the potential in volts, E∘ is the standard potential at 25 ∘C in volts, R=8.314J/(K⋅mol) is the gas constant, T is the temperature in kelvins, n is the number of moles of electrons transferred, F=96,500C/(mol e−) is the Faraday constant, and Q is the reaction quotient. At the common reference temperture of 298 K, substituting each constant into the equation the result is E=E∘−(0.0592 V/n)log10Q a) Calculate the standard cell potential at 25 ∘C for Mg(s)+Fe2+(aq)→Mg2+(aq)+Fe(s) b) What is the cell potential for the reaction Mg(s)+Fe2+(aq)→Mg2+(aq)+Fe(s) at 57 ∘C when [Fe2+]= 3.80 MM and [Mg2+]= 0.210 MM .
ANSWER ASAP PLEASE THANK U What is the Eo for the cell: L | L2+(aq) || T2+(aq) | T ? Final answer: two decimal places; include negative sign whenever applicable; no unit necessary. Use data given in Table 1. Table 1. Standard Reduction Potentials at 25oC of Some Hypothetical Substances A3+ + 3e- → A Eo = + 1.4 V X2+ + 2e- → X Eo = - 2.87 V R3+ + e- → R2+ Eo = + 0.77 V J2 + 2e- → 2J- Eo = + 0.54 V L2+ + 2e- → L Eo = - 1.78 V T2+ + 2e- → T Eo = - 0.23 V
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