Recent questions in ElectroChemistry

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1 answer 46 views

A student wanted to determine the Faraday constant using the electrolysis of silver nitrate solution. If a current of 2.5 amperes flowed through the solution for 2 hours and 30 minutes, and 0.508 grams of silver were deposited on the cathode, what is the value of the Faraday constant?

asked Jan 22 in ElectroChemistry by YWYElizbeth9 (810 points)

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1 answer 35 views

A student sets up an electrochemical cell with two copper electrodes and a copper(II) sulfate solution. The concentration of the copper(II) sulfate solution is 0.1 M. The student measures the potential difference between the electrodes as 0.54 V. Calculate the resistance of the cell in ohms.

asked Jan 22 in ElectroChemistry by BlancaHaigle (690 points)

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1 answer 60 views

A student needs to determine the standard electrode potential for the following reaction: Fe3+ + e- → Fe2+ Using the standard electrode potentials of Fe3+/Fe2+ and Ag+/Ag, calculate the standard cell potential for the following reaction: 2Ag+ (aq) + Fe(s) → 2Ag(s) + Fe2+ (aq) Determine if this reaction is spontaneous or nonspontaneous under standard conditions.

asked Jan 22 in ElectroChemistry by SpencerRagga (790 points)

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1 answer 71 views

A student needs to determine the mass of silver that can be deposited on a silver electrode using a current of 2.5 A for 3 hours in a solution containing 0.2 M silver ions. What is the mass of silver deposited on the electrode? (Assuming 100% current efficiency and atomic weight of silver is 107.9 g/mol)

asked Jan 22 in ElectroChemistry by HalWhitten9 (590 points)

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1 answer 6 views

A student needs to determine the activation energy for the electrochemical reaction between zinc and copper sulfate using the Arrhenius equation. The student has experimental data that includes the rate constants and temperatures at which the reaction was performed. Using the experimental data, the student needs to calculate the activation energy for the reaction and explain the significance of this value in terms of the reaction kinetics.

asked Jan 22 in ElectroChemistry by OllieGirardi (210 points)

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1 answer 36 views

A student needs to determine the activation energy for an electrochemical reaction involving the oxidation of Zinc using a voltage of 1.85V, a current of 0.25A and a temperature of 25°C. Given that the standard potential for this reaction at 25°C is -0.76V, what is the activation energy of the reaction?

asked Jan 22 in ElectroChemistry by GiaMelendez4 (370 points)

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1 answer 51 views

A student needs to calculate the Tafel slopes for the anodic and cathodic reactions from a given set of experimental data obtained during an electrochemical experiment. The experiment involves the corrosion of iron in a solution with a pH of 3.5. The anodic and cathodic current densities were measured at various applied potentials ranging from -700 mV vs SHE to -400 mV vs SHE. The student needs to plot a Tafel plot for each reaction and calculate their corresponding Tafel slopes. Based on the obtained results, the student needs to explain the corrosion mechanism of iron in the given acidic solution.

asked Jan 22 in ElectroChemistry by AveryCoughli (450 points)

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1 answer 78 views

A student needs to calculate the resistance of an electrochemical cell that has a concentration of 0.1 M for both copper(II) and zinc(II) ions, using an electrochemical sensor that measures 2.5 volts for the cell. Calculate the resistance of the electrochemical cell at room temperature, given that the Faraday constant is 96485 C/mol and the gas constant is 8.314 J/(mol·K).

asked Jan 22 in ElectroChemistry by LindseyTulk (330 points)

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1 answer 46 views

A student needs to calculate the maximum electrical work that can be obtained from an electrochemical cell of standard hydrogen electrode (SHE) potential -0.76 V and a zinc electrode potential of -0.46 V, when 0.5 moles of zinc metal is oxidized to form zinc ions at 25 °C. Assume that the Faraday constant is 96,485 Coulombs per mole of electrons and the gas constant is 8.314 J/mole.K.

asked Jan 22 in ElectroChemistry by StewartLivin (490 points)

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1 answer 48 views

A student needs to calculate the Faraday constant for the reduction of copper ions in a solution using a current of 2.5 amperes for 5 minutes. If the mass of copper deposited on the cathode was 0.3 grams, what is the value of the Faraday constant?

asked Jan 22 in ElectroChemistry by IrvinLeichha (410 points)

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1 answer 49 views

A student needs to calculate the efficiency of an electrochemical cell that has a potential difference of 1.5 volts and a current of 0.5 amperes passing through it, with the help of Faraday's Law. If the electrode reaction produces chlorine gas with a Faraday efficiency of 79%, and the overall voltage efficiency of the cell is 85%, what is the efficiency of the electrochemical cell?

asked Jan 22 in ElectroChemistry by DevonGreeves (390 points)

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1 answer 39 views

A student needs to calculate the efficiency of a voltaic cell that has a standard potential difference of 0.78 V and produces a current of 2.5 A. The cell is operated for 8 hours and consumes a total of 2400 Coulombs of charge. What is the efficiency of this electrochemical cell?

asked Jan 22 in ElectroChemistry by LinoLadd0317 (400 points)

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1 answer 77 views

A student needs to calculate the current density (in Amperes per square meter) of a copper electrode (Area = 10 cm²) in an electrochemical cell where the half-cell reaction is Cu²⁺ + 2e⁻ → Cu and the cell voltage is 1.1 V. The concentration of Cu²⁺ in the cell is 0.1 M.

asked Jan 22 in ElectroChemistry by Christiane98 (390 points)

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1 answer 47 views

A student needs to calculate the current density (in A/m^2) in an electrochemical cell with a cross-sectional area of 0.01 m^2 and a current of 0.5 A passing through it. The half-cell reactions are as follows:Anode: Zn(s) -> Zn2+(aq) + 2e^-Cathode: Cu2+(aq) + 2e^- -> Cu(s)The concentrations of Zn2+ and Cu2+ ions in the solutions are 0.1 M and 0.01 M, respectively. The temperature of the cell is 298 K. Calculate the current density.

asked Jan 22 in ElectroChemistry by ShellyGiron1 (410 points)

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1 answer 56 views

A student needs to calculate the activation energy for a reaction that takes place at an electrode with a current density of 2.5 mA/cm² at a temperature of 25°C. The reaction has a transfer coefficient of 0.5 and a standard rate constant of 2.0 × 10⁻⁶ cm/s. The student has access to the necessary thermodynamic data for the reaction. What is the activation energy for this electrochemical reaction?

asked Jan 22 in ElectroChemistry by ShaniGrondin (630 points)

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1 answer 68 views

A student measures the current in a galvanic cell with a standard potential of 1.10 V, using a Zinc electrode and a Copper electrode. The student recorded the current as 0.50 A. What is the rate of the electrochemical reaction occurring in the cell?

asked Jan 22 in ElectroChemistry by StephanyWurs (470 points)

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1 answer 76 views

A student is studying the overpotential in an electrochemical reaction in a laboratory experiment. The student measures a current of 2.1 A at an electrode potential of -0.6 V, and 1.95 A at -0.5 V. What is the overpotential of the reaction?

asked Jan 22 in ElectroChemistry by LancePrenzel (510 points)

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1 answer 71 views

A student is studying the electrochemical reaction of the metal copper in acidic solution. They measure the current density at different applied potentials and obtain the following data:Potential vs. SHE (V) | Current Density (mA/cm²)---|---0.0 | 0.00.1 | 0.50.2 | 2.00.3 | 5.00.4 | 11.0Using this data, calculate the anodic and cathodic Tafel slopes, and determine the rate constant for the electrochemical reaction.

asked Jan 22 in ElectroChemistry by ZPTCarole74 (510 points)

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1 answer 51 views

A student is studying the electrochemical behavior of a certain metal ion in a solution of varying pH values. They have measured the anodic and cathodic Tafel slopes for the electrode reaction at each pH. The anodic Tafel slope values range from 60 mV/decade to 90 mV/decade, and the corresponding cathodic Tafel slope values range from 50 mV/decade to 70 mV/decade. Is this metal ion undergoing a one-electron or a two-electron transfer reaction? Justify your answer.

asked Jan 22 in ElectroChemistry by ColumbusRebe (830 points)

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1 answer 56 views

A student is given the electrochemical cell reaction:MnO4-(aq) + 8H+(aq) + 5e- → Mn2+(aq) + 4H2O(l)Calculate the standard potential (in volts) of the cell at 25°C given that the standard reduction potential of MnO4-(aq)/Mn2+(aq) couple and the standard reduction potential of the H+(aq)/H2(g) couple are +1.51 V and 0.00 V, respectively. The concentration of MnO4-(aq) is 0.010 M and that of H+(aq) is 1.00 M.

asked Jan 22 in ElectroChemistry by MistyCordeau (530 points)

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