Recent questions in ElectroChemistry

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Calculate the cell potential for the following galvanic cell where a nickel anode is placed in a 1.0M Ni(NO3)2 solution and a silver cathode is placed in a 1.0M AgNO3 solution. The balanced equation for the cell reaction is: Ni(s) + 2 Ag+(aq) → Ni2+(aq) +2 Ag(s) Assume that standard reduction potentials for each half-reaction are as follows: Ni2+(aq) + 2 e- ⇌ Ni(s) E° = -0.25V Ag+(aq) + e- ⇌ Ag(s) E° = +0.80V What is the cell potential at standard conditions (25°C and 1 atm)?

asked Jan 23 in ElectroChemistry by GermanFranki (1.8k points)

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1 answer 110 views

Calculate the cell potential for the following electrochemical reaction:Zn(s) + Cu2+(aq) → Zn2+(aq) + Cu(s)Given that the standard reduction potentials for the half-reactions are as follows:Zn2+(aq) + 2e- → Zn(s) E° = -0.76 VCu2+(aq) + 2e- → Cu(s) E° = +0.34 V

asked Jan 23 in ElectroChemistry by TobiasTudawa (1.9k points)

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Calculate the cell potential for the following electrochemical reaction: Cu(s) + 2 Ag+(aq) → Cu2+(aq) + 2 Ag(s) The standard reduction potentials are: Cu2+(aq) + 2 e- → Cu(s) E° = 0.34 V Ag+(aq) + e- → Ag(s) E° = 0.80 V

asked Jan 23 in ElectroChemistry by FinleySalern (1.6k points)

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Calculate the cell potential for the following electrochemical reaction: Cu(s) + 2 Ag⁺(aq) → Cu²⁺(aq) + 2 Ag(s) Given that the standard reduction potentials are: Cu²⁺(aq) + 2e⁻ → Cu(s) E° = +0.34 V Ag⁺(aq) + e⁻ → Ag(s) E° = +0.80 V

asked Jan 23 in ElectroChemistry by AundreaWhitf (1.8k points)

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1 answer 96 views

Calculate the cell potential for the following electrochemical reaction at 25°C: Zn(s) + 2AgNO3(aq) → Zn(NO3)2(aq) + 2Ag(s) Given: E°(Ag+/Ag) = +0.80 V E°(Zn2+/Zn) = −0.76 V

asked Jan 23 in ElectroChemistry by Lynell160113 (1.8k points)

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1 answer 107 views

Calculate the cell potential for a given electrochemical reaction where the half-cell reactions are:* Fe3+(aq) + e- → Fe2+(aq) E° = 0.77 V* Ag+(aq) + e- → Ag(s) E° = 0.80 VAssume 1.0 M solutions and standard state conditions. Determine whether the reaction is spontaneous or non-spontaneous under standard conditions.

asked Jan 23 in ElectroChemistry by AntoniettaLa (1.9k points)

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1 answer 129 views

Calculate the cell potential at standard conditions for the electrochemical reaction: Cu(s) + 2Ag+(aq) -> 2Ag(s) + Cu2+(aq) given that the standard reduction potentials for Cu2+(aq)/Cu(s) and Ag+(aq)/Ag(s) are +0.34 V and +0.80 V, respectively.

asked Jan 23 in ElectroChemistry by MoniqueBrins (1.9k points)

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Calculate the anodic Tafel slope for the following electrochemical reaction taking place at a platinum electrode:Fe2+(aq) + 2e- → Fe(s) Given that the exchange current density is 4.50 x 10^-4 A/cm^2 and the reaction rate constant for the reaction is 2.5 x 10^5 cm/s.

asked Jan 23 in ElectroChemistry by DeanI7567799 (2.2k points)

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1 answer 102 views

Calculate the anodic Tafel slope for an electrochemical cell in which the corrosion current density is 0.05 mA/cm² and the anodic overpotential is 50 mV. The exchange current density for the anodic reaction is 0.02 mA/cm².

asked Jan 23 in ElectroChemistry by OrvalLasley3 (2.1k points)

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1 answer 45 views

Calculate the anodic Tafel slope for a reaction with an exchange current density of 2x10^-4 A cm^-2 if the current density at an anodic potential of 0.1V vs the standard hydrogen electrode (SHE) is 0.5 mA cm^-2 and at 0.2V vs SHE is 2.0 mA cm^-2. Assume a linear relationship between current density and overpotential.

asked Jan 23 in ElectroChemistry by RudyMms5536 (1.8k points)

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1 answer 104 views

Calculate the anodic Tafel slope (in mV/decade) for the corrosion of iron in a solution containing 0.1 M HCl, given that the corrosion current density is 2.5 mA/cm2 and the exchange current density is 0.25 mA/cm2. Assume T = 25°C and the activation energy of the reaction is 40 kJ/mol.

asked Jan 23 in ElectroChemistry by ErnestinaMus (1.9k points)

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1 answer 102 views

Calculate the amount of copper deposited on the cathode when a current of 5 amperes is passed through a copper sulfate solution for a duration of 30 minutes. The molar mass of copper is 63.55 g/mol and the Faraday constant is 96500 C/mol. The electrode area is 10 cm² and the copper sulfate solution has a concentration of 0.1 M. Assume 100% efficiency in the electrochemical reaction.

asked Jan 23 in ElectroChemistry by ChristianeBo (2.0k points)

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1 answer 154 views

Calculate the activation energy of the following electrochemical reaction: 2Fe^3+(aq) + 2I^-(aq) → 2Fe^2+(aq) + I2(s) Given that the reaction rate constant at 25°C is 1.0 × 10^-3 s^-1, and the reaction's activation energy follows the Arrhenius equation with a pre-exponential factor of 8.0 × 10^7 s^-1.

asked Jan 23 in ElectroChemistry by MartyKindler (1.5k points)

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1 answer 99 views

Calculate the activation energy for the following electrochemical reaction: 2H₂O(l) → O₂(g) + 4H⁺(aq) + 4e⁻ if the half-cell potentials are: E°(O₂/H₂O) = 1.23 V E°(H⁺/H₂) = 0 V Assuming the reaction follows Arrhenius equation, where the rate constant k is related to the activation energy Ea, temperature T and pre-exponential factor A by: k = A exp(-Ea/RT) where R is the gas constant equal to 8.314 J/molK.

asked Jan 23 in ElectroChemistry by ShaunBehan45 (2.8k points)

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1 answer 91 views

Calculate the activation energy for the electrochemical reaction of zinc and copper sulfate solution using the slope of the Tafel plot obtained from the data collected during a cyclic voltammetry experiment.

asked Jan 23 in ElectroChemistry by IFYRussel191 (2.2k points)

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1 answer 96 views

At 25°C, an electrochemical cell consists of a silver electrode in a 0.010 M AgNO3 solution and a platinum electrode in a 1.0 x 10^-3 M HCl solution. Calculate the resistance of the cell if the distance between the two electrodes is 2.0 cm and the area of each electrode is 5.0 cm^2.

asked Jan 22 in ElectroChemistry by REHJon915716 (1.9k points)

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1 answer 110 views

Assuming that the concentration of Cu2+ ions in a solution is 0.25 M, the concentration of Ag+ ions in another solution is 0.50 M, and the standard reduction potential of Cu2+(aq) + 2e- → Cu(s) is +0.34 V and that of Ag+(aq) + e- → Ag(s) is +0.80 V, calculate the current density when the two solutions are separated by a salt bridge and connected by a wire.

asked Jan 22 in ElectroChemistry by MercedesLang (2.2k points)

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1 answer 115 views

Assuming a standard hydrogen electrode is used as the reference electrode and a copper electrode is used as the working electrode in an electrochemical cell, calculate the polarization potential when the current density on the copper electrode is 0.5 mA/cm^2 and the concentration of Cu2+ in the solution is 0.1 M.

asked Jan 22 in ElectroChemistry by MelbaTulloch (2.2k points)

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1 answer 91 views

An electrochemical cell has a standard emf of 1.10 V and a current of 0.500 A when operating at standard conditions. What is the power output of the cell?

asked Jan 22 in ElectroChemistry by FinleySalern (1.6k points)

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1 answer 96 views

An aqueous solution of 1.0 M HCl is oxidized by a lead anode in a half-cell, while a half-cell with a hydrogen electrode is used as the standard reduction potential. If the electrode potential of the lead electrode is -0.13 V, what is the cell potential of the overall reaction?

asked Jan 22 in ElectroChemistry by OrenTherrien (1.8k points)

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