Recent questions in ElectroChemistry

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What is the rate of electroplating in a cell with a current of 2.5 A passing through it for 1 hour if the mass of the metal deposited on the cathode is 0.456 g? (assume a 100% yield and use the appropriate formula to calculate the rate).

asked Mar 1 in ElectroChemistry by TheScientist (138k points)

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What is the power output of an electrochemical cell with a standard potential of +0.34 V and a current of 2.5 A flowing through it for 3 hours?

asked Mar 1 in ElectroChemistry by TheScientist (138k points)

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What is the power output (in Watts) of an electrochemical cell at standard conditions, given that the cell potential is 1.5V and the total resistance of the circuit is 10 ohms?

asked Mar 1 in ElectroChemistry by TheScientist (138k points)

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What is the polarization in an electrochemical cell when the current density is 200 A/m², the effective surface area of the electrode is 50 cm², the electrode potential is -0.5V and the electrolyte resistance is 10 Ω?

asked Mar 1 in ElectroChemistry by TheScientist (138k points)

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What is the maximum power output of a galvanic cell consisting of a zinc electrode and a copper electrode, with a concentration of 0.1 M Zn2+ and 0.01 M Cu2+? Assume a standard hydrogen electrode (SHE) as the reference electrode and a temperature of 25°C.

asked Mar 1 in ElectroChemistry by TheScientist (138k points)

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How much mass of silver (Ag) will be deposited onto a cathode during the electrolysis of a silver nitrate (AgNO3) solution using a current of 2.5 A for 20 minutes? The molar mass of silver is 107.868 g/mol and the Faraday constant is 96,485 C/mol.

asked Mar 1 in ElectroChemistry by TheScientist (138k points)

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What is the mass of copper deposited on a cathode when a current of 5A is applied for 1 hour in a copper sulfate solution with a concentration of 0.5M? (Molar Mass of Cu: 63.55 g/mol and Faraday's constant: 96,485 C/mol)

asked Mar 1 in ElectroChemistry by TheScientist (138k points)

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What is the mass of copper deposited on the cathode when a current of 5 A is passed through a solution of copper (II) sulfate for 2 hours? Given that the atomic mass of copper is 63.5 g/mol and the Faraday constant is 96485 C/mol.

asked Mar 1 in ElectroChemistry by TheScientist (138k points)

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What is the mass of aluminum metal that can be deposited by passing a current of 5.0 A through an Al(NO3)3 solution for 45 minutes? (Assume 100% efficiency and a Faraday constant of 96,500 C/mol.)

asked Mar 1 in ElectroChemistry by TheScientist (138k points)

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What is the Gibbs free energy change at 298 K for the reaction 2Fe2+(aq) + Cl2(g) --> 2Fe3+(aq) + 2Cl-(aq) if the standard electrode potentials for the half-reactions are E°(Fe3+(aq) + e- --> Fe2+(aq)) = -0.77 V and E°(Cl2(g) + 2e- --> 2Cl-(aq)) = 1.36 V?

asked Mar 1 in ElectroChemistry by TheScientist (138k points)

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What is the Gibbs free energy change for the electrochemical reaction:Zn(s) + Cu2+(aq) → Zn2+(aq) + Cu(s)given that the standard reduction potentials are E°(Cu2+|Cu) = +0.34 V and E°(Zn2+|Zn) = -0.76 V, and the reaction is carried out at 25°C?

asked Mar 1 in ElectroChemistry by TheScientist (138k points)

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What is the Gibbs free energy change of a spontaneous electrochemical reaction where zinc metal electrode is used as an anode and copper metal electrode is used as a cathode, with a cell potential of 1.10 V?

asked Mar 1 in ElectroChemistry by TheScientist (138k points)

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What is the Gibbs free energy change for the reaction of Zinc with Copper sulfate solution in which Zinc gets oxidized to Zinc sulfate and Copper ions get reduced to Copper metal, given the standard reduction potentials for each half-reaction?

asked Mar 1 in ElectroChemistry by TheScientist (138k points)

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What is the Gibbs free energy change for the electrochemical reduction of 1 mol of Au3+ to Au in a standard electrochemical cell with a cell potential of 1.42 V at 298 K?

asked Mar 1 in ElectroChemistry by TheScientist (138k points)

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What is the Gibbs free energy change for the electrochemical reaction involving the oxidation of copper, Cu, to copper (II) ions, Cu2+, in a solution of CuSO4 with a potential of 0.78 V at 25°C?

asked Mar 1 in ElectroChemistry by TheScientist (138k points)

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What is the Gibbs free energy change for the electrochemical reaction when a copper electrode is placed in a 1 M copper(II) sulfate solution and a standard hydrogen electrode (SHE) is placed in a 1 M hydrogen ion solution at 25°C?

asked Mar 1 in ElectroChemistry by TheScientist (138k points)

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In an electrochemical experiment, the anodic and cathodic Tafel slopes were found to be 100 mV/decade and 120 mV/decade, respectively. Calculate the value of exchange current density for the reaction.

asked Mar 1 in ElectroChemistry by TheScientist (138k points)

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What is the exchange current density (in A/cm2) for the reaction 2H+ + 2e- ⇌ H2 at a temperature of 298 K and a concentration of 0.1 M H+? Given that the standard potential of the half-cell reaction is 0 V, and the Tafel slope is 60 mV/decade.

asked Mar 1 in ElectroChemistry by TheScientist (138k points)

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1 answer 37 views

What is the exchange current density for the oxidation of iron in a 0.1 M solution of Fe2+/Fe3+ at 25°C if the standard potential of the couple is +0.77 V and the overpotential is 0.2 V?

asked Mar 1 in ElectroChemistry by TheScientist (138k points)

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What is the exchange current density for the oxidation of iron in a 0.1 M Fe2+(aq) solution at 25°C, assuming the standard electrode potential for the Fe2+/Fe3+ couple is +0.77 V? The rate constant for the reaction is 1.2x10^-5 cm/s.

asked Mar 1 in ElectroChemistry by TheScientist (138k points)

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