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Recent questions in ElectroChemistry
0
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1
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Calculate the exchange current density of a copper-copper(II) ion electrode at 25 °C, given that the standard potential of the electrode is +0.34 V versus the standard hydrogen electrode and the transfer coefficient of the electrode reaction is 0.5.
asked
Jan 23
in
ElectroChemistry
by
AlexK0785479
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1.8k
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0
votes
1
answer
60
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Calculate the exchange current density for the redox reaction: Fe2+ + Cr2O72- + 14H+ → 2Fe3+ + 2Cr3+ + 7H2O Given that the standard potential for the reaction at 25°C is 1.33 V, the gas constant is 8.314 J/mol K, and the temperature is 298 K.
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Jan 23
in
ElectroChemistry
by
DarbyJackey7
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1.4k
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0
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1
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60
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Calculate the exchange current density for a Zinc electrode immersed in a solution containing 0.1 M Zinc ions at 25 degrees Celsius, given that the standard potential of the Zinc half-reaction is -0.76 V and the transfer coefficient is 0.5. (Assume concentration polarization effects to be negligible.)
asked
Jan 23
in
ElectroChemistry
by
KassieStarns
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2.3k
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0
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1
answer
42
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Calculate the exchange current density for a zinc electrode immersed in a 1.0 M solution of zinc sulfate at 25°C when the overpotential is 0.05 V. The standard reduction potential for the Zn2+/Zn couple is -0.76 V. The transfer coefficient is 0.5. Assume that the concentration of the electrolyte does not change significantly during the reaction.
asked
Jan 23
in
ElectroChemistry
by
TroyWitcher8
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2.1k
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0
votes
1
answer
78
views
Calculate the exchange current density for a redox reaction where the standard potential is 0.7 V, and the transfer coefficient is 0.5, given that the rate constant for the reaction is 5 × 10^-7 mol/cm^2*s.
asked
Jan 23
in
ElectroChemistry
by
AndrewSisley
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2.1k
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votes
1
answer
76
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Calculate the exchange current density for a metal electrode immersed in a 1 M solution of its corresponding ions. The standard rate constant for the reaction is 6.3 x 10^-5 cm/s and the concentration of the electrons in the electrode is 5 x 10^23 atoms/cm^3. Additionally, assume the temperature is 25°C and the Faraday constant is 96,500 C/mol.
asked
Jan 23
in
ElectroChemistry
by
Leif76792351
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2.0k
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0
votes
1
answer
65
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Calculate the exchange current density at the interface between a silver electrode and an aqueous solution of silver ions, given that the standard reduction potential for the Ag+/Ag half-cell is +0.80 V, the concentration of Ag+ in the solution is 0.025 M, and the temperature is 25°C.
asked
Jan 23
in
ElectroChemistry
by
CornellNicho
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2.1k
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0
votes
1
answer
97
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Calculate the exchange current density at the cathode of a lithium-ion battery if the temperature of the battery is 25 °C, the standard potential of
asked
Jan 23
in
ElectroChemistry
by
OnitaLoftus1
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2.3k
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0
votes
1
answer
69
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Calculate the equilibrium constant, K, for the electrochemical reaction below, given the standard reduction potentials at 298 K:2 H+ (aq) + 2 e- → H2 (g) E° = 0.00 VFe3+ (aq) + e- → Fe2+ (aq) E° = +0.771 V
asked
Jan 23
in
ElectroChemistry
by
TroyPurton77
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1.9k
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0
votes
1
answer
79
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Calculate the equilibrium constant for the reaction that occurs when a copper electrode is placed in a solution of 0.1 M copper(II) sulfate and connected to a standard hydrogen electrode. The cell potential at standard conditions is observed to be 0.34 V. (Hint: Use the Nernst equation to relate the cell potential to the equilibrium constant.)
asked
Jan 23
in
ElectroChemistry
by
YvetteLink0
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2.0k
points)
0
votes
1
answer
74
views
Calculate the equilibrium constant for the following electrochemical reaction at a temperature of 25°C:$$\ce{Co^{2+} + 2e^- <=> Co(s)}$$Given that the standard reduction potential for the half-reaction is $-0.28\,\text{V}$ and the concentration of $\ce{Co^{2+}}$ is $0.1\,\text{M}$.
asked
Jan 23
in
ElectroChemistry
by
Shawn33B4717
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1.9k
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0
votes
1
answer
83
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Calculate the equilibrium constant for the following electrochemical reaction at 298K:$$\ce{2Fe^3+ (aq) + 2I^- (aq) -> 2Fe^2+ (aq) + I2 (s)}$$ Given: Standard reduction potentials: $\ce{Fe^3+ + e^- -> Fe^2+}$ Eº = +0.77V $\ce{2I^- -> I2 + 2e^- }$ Eº = +0.54V
asked
Jan 23
in
ElectroChemistry
by
Ben56061281
(
1.4k
points)
0
votes
1
answer
68
views
Calculate the equilibrium constant for the following electrochemical cell reaction at 25°C:Cu(s) + 2 Ag+(aq) --> Cu2+(aq) + 2 Ag(s)Given the standard reduction potentials are:Cu2+(aq) + 2 e- → Cu(s) E°red = +0.34 VAg+(aq) + 1 e- → Ag(s) E°red = +0.80 V
asked
Jan 23
in
ElectroChemistry
by
DeenaKuhn606
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2.0k
points)
0
votes
1
answer
80
views
Calculate the equilibrium constant for the electrochemical reaction: Zn(s) + 2H^+(aq) → Zn^2+(aq) + H2(g) when the concentration of Zn^2+ is 0.25 M, [H^+] is 2.5 × 10^-3 M, and the pressure of H2 is 0.8 atm at 298 K.
asked
Jan 23
in
ElectroChemistry
by
GiselleDange
(
1.6k
points)
0
votes
1
answer
76
views
Calculate the equilibrium constant for the electrochemical cell reaction given below, if the standard reduction potential for the reduction of Fe3+ ion is -0.771 V and for the reduction of Ag+ ion is +0.799 V. Fe3+ + 3e- → Fe (s) E° = -0.771 VAg+ + e- → Ag (s) E° = +0.799 V
asked
Jan 23
in
ElectroChemistry
by
JonasOql0066
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1.5k
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0
votes
1
answer
82
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Calculate the equilibrium constant (K) of the electrochemical reaction below at 298K:Fe(s) + Cu2+(aq) ⇌ Fe2+(aq) + Cu(s) Given that at standard state (1 atm and 298K) the standard reduction potentials of Fe2+(aq)/Fe(s) and Cu2+(aq)/Cu(s) are -0.44 V and +0.34 V, respectively.
asked
Jan 23
in
ElectroChemistry
by
LibbyHollera
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2.4k
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0
votes
1
answer
63
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Calculate the equilibrium constant (K) of the electrochemical reaction below at 25°C: 2AgCl(s) + H2(g) <--> 2Ag(s) + 2HCl(aq) Given: E°AgCl/Ag = 0.22 V E°HCl/H2 = 0.00 V Kw = 1.0 x 10^-14 at 25°C Standard Hydrogen Electrode (SHE) has E° = 0.00 V
asked
Jan 23
in
ElectroChemistry
by
QJXClarice2
(
2.5k
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0
votes
1
answer
81
views
Calculate the equilibrium constant (K) for the reaction that occurs when a nickel electrode is placed in a solution containing 1.0 M of nickel ions and 1.0 M of copper ions. The nickel electrode was placed in the solution, and the cell potential was measured to be 0.21 V at 25 °C.
asked
Jan 23
in
ElectroChemistry
by
CorneliusU11
(
1.7k
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0
votes
1
answer
70
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Calculate the equilibrium constant (K) for the reaction between copper and silver ions in a galvanic cell at room temperature (25°C), given the following half-reactions and their respective reduction potentials:Cu2+ (aq) + 2e- → Cu (s) E°red = +0.34 VAg+ (aq) + e- → Ag (s) E°red = +0.80 VAlso, if the cell is constructed with a copper electrode and a silver electrode, which electrode will be the cathode and which will be the anode?
asked
Jan 23
in
ElectroChemistry
by
RandellBeggs
(
2.0k
points)
0
votes
1
answer
72
views
Calculate the equilibrium constant (K) for the electrochemical reaction: Mg(s) + 2 Ag+(aq) → Mg2+(aq) + 2 Ag(s) Given that the standard reduction potentials for Ag+ and Mg2+ are +0.80 V and -2.37 V, respectively. The concentration of Ag+ is 0.020 M and the concentration of Mg2+ is 0.080 M.
asked
Jan 23
in
ElectroChemistry
by
DaleHaveman
(
2.1k
points)
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