Recent questions in ElectroChemistry

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1 answer 78 views

Here is a precise question for the student to solve:A student performed an electroplating experiment of copper metal onto an electrode by passing a constant current of 1.5 A through a solution of copper(II) sulfate for 50 minutes. If the mass of the copper metal obtained was 1.23 grams, calculate the Faraday constant using the following formula: Faraday constant = (mass of substance plated x molar mass of substance) / (current x time)

asked Feb 4 in ElectroChemistry by KreogMoore5 (6.4k points)

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1 answer 48 views

Here is a precise problem for the student to solve:A copper electrode is placed in a solution of copper nitrate with a concentration of 0.1 M, while a platinum electrode is placed in a solution of hydrogen peroxide. The potential difference of the half-reactions for the copper/copper(II) and hydrogen peroxide/water couples are +0.34 V and +1.77 V, respectively. Calculate the current density (in A/m²) at the copper electrode when a current of 0.25 A is passed through the cell for 10 minutes.

asked Feb 4 in ElectroChemistry by HarryHodgkin (2.2k points)

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1 answer 70 views

Given the following reaction at standard conditions:Cu(s) + 2Ag+(aq) -> Cu2+(aq) + 2Ag(s) Calculate the cell potential, E°cell, at 25°C using the standard reduction potentials:Cu2+(aq) + 2e- -> Cu(s), E°red = +0.34 VAg+(aq) + e- -> Ag(s), E°red = +0.80 V

asked Feb 4 in ElectroChemistry by Phillipp57B1 (2.3k points)

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1 answer 84 views

Given the following half-reactions:Cu²⁺ (aq) + 2e⁻ → Cu (s) E° = +0.34 VAg⁺ (aq) + e⁻ → Ag (s) E° = +0.80 VWhat is the cell potential for the reaction when a copper electrode is paired with a silver electrode in a standard electrochemical cell?

asked Feb 4 in ElectroChemistry by ElyseY075419 (1.7k points)

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1 answer 46 views

Given the following half-reactions:Cu2+ (aq) + 2 e- -> Cu (s) E° = +0.34 VZn2+ (aq) + 2 e- -> Zn (s) E° = -0.76 VCalculate the equilibrium constant (K) for the reaction: Cu2+ (aq) + Zn (s) -> Zn2+ (aq) + Cu (s)

asked Feb 4 in ElectroChemistry by AndreasLdp14 (1.7k points)

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1 answer 84 views

Given the following electrochemical reaction: Cu(s) + 2 Ag+(aq) → Cu2+(aq) + 2 Ag(s)Calculate the cell potential at standard conditions (298 K, 1 atm, 1 M concentrations).

asked Feb 4 in ElectroChemistry by ChasityBelli (2.2k points)

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1 answer 62 views

Given the following electrochemical equation:Cu(s) | Cu²⁺(aq, 0.0100 M) || Cr³⁺(aq, 1.00 M) | Cr(s)At 298 K, the standard reduction potential for Cu²⁺/Cu is +0.34 V and for Cr³⁺/Cr is -0.74 V. Calculate the equilibrium constant (K) for the above electrochemical reaction.

asked Feb 4 in ElectroChemistry by AlfonsoJanze (1.9k points)

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1 answer 76 views

Given the following data for the electrochemical reaction A + B → C, where A and B are electrons:- The anodic Tafel slope is 50 mV per decade of current density.- The cathodic Tafel slope is 70 mV per decade of current density.Calculate the exchange current density (i0) for the reaction.

asked Feb 4 in ElectroChemistry by CarltonWoote (1.7k points)

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1 answer 76 views

Given the electrochemical reaction Zn(s) + Cu2+(aq) → Zn2+(aq) + Cu(s), calculate the standard cell potential at 25°C if the standard reduction potentials are E°(Cu2+/Cu) = 0.34 V and E°(Zn2+/Zn) = -0.76 V.

asked Feb 4 in ElectroChemistry by HIELucille73 (2.1k points)

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1 answer 68 views

Given the balanced equation for the electrochemical reaction: Cu(s) + 2AgNO3(aq) → Cu(NO3)2(aq) + 2Ag(s)Calculate the number of electrons transferred per copper atom during this reaction when a current of 5.00 A is passed for 6.00 minutes through a cell containing a copper electrode and a silver electrode with a silver ion concentration of 0.100 M.

asked Feb 4 in ElectroChemistry by HarleyOreill (1.9k points)

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1 answer 77 views

Given a half-reaction Cu2+(aq) + 2e- --> Cu(s) with an electrode potential of +0.34V and a half-reaction Fe3+(aq) + e- --> Fe2+(aq) with an electrode potential of +0.77V, what is the cell potential for the electrochemical reaction when Cu2+(aq) and Fe3+(aq) ions react to form Cu(s) and Fe2+(aq) ions?

asked Feb 4 in ElectroChemistry by EttaRide758 (1.3k points)

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1 answer 117 views

Given a certain electrochemical reaction, the anodic and cathodic Tafel slopes were found to be 60 mV/decade and 100 mV/decade, respectively. Calculate the exchange current density of the reaction.

asked Feb 4 in ElectroChemistry by Francisca504 (1.9k points)

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1 answer 74 views

For the reaction below, calculate the equilibrium constant (K) when the electrode potentials are E°(Cu2+/Cu) = +0.34 V and E°(Ag+/Ag) = +0.80 V:Cu(s) + 2Ag+(aq) → Cu2+(aq) + 2Ag(s)

asked Feb 4 in ElectroChemistry by HalinaAlderm (1.9k points)

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1 answer 93 views

For the electrochemical reaction + ↔ + , the cell potential is 0.60 V at 25°C. If the standard reduction potential of 2+ is 0.34 V and that of 2+ is -0.74 V, calculate the equilibrium constant () for the reaction at 25°C.

asked Feb 4 in ElectroChemistry by TracieM73151 (2.5k points)

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1 answer 62 views

Determine the Tafel slopes for the oxidation of H2 gas and the reduction of O2 gas using a platinum electrode in a 1 M acidic solution. The measured current densities at the anode and cathode were 0.5 mA/cm² and 0.3 mA/cm², respectively.

asked Feb 4 in ElectroChemistry by AudraNowlin6 (2.2k points)

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1 answer 64 views

Determine the oxidation state of the following elements in the compound potassium permanganate (KMnO4): a) Potassium b) Manganese c) Oxygen

asked Feb 4 in ElectroChemistry by Annett65L392 (2.1k points)

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1 answer 89 views

Determine the oxidation state of sulfur in sodium sulfite (Na2SO3) using the oxidation state rules and justify your answer with proper explanation.

asked Feb 4 in ElectroChemistry by JeroldStonem (1.6k points)

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1 answer 74 views

Determine the number of electrons transferred in the following electrochemical reaction: Cu(s) + 2Ag+(aq) → Cu2+(aq) + 2Ag(s) Show the calculation steps and write the balanced half-reactions with the number of electrons transferred.

asked Feb 4 in ElectroChemistry by BrandieB8434 (2.2k points)

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1 answer 70 views

Determine the corrosion current density of a copper plate in a 0.1 M NaCl solution at 25°C, given that the corrosion potential of the copper plate in the solution is -0.54 V vs. the standard hydrogen electrode (SHE) and the Tafel slope for copper in the solution is 120 mV/decade.

asked Feb 4 in ElectroChemistry by LynwoodLundg (1.5k points)

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1 answer 101 views

Determine the activation energy for the electrochemical reaction that occurs between copper and nitric acid (Cu + 4HNO3 --> Cu(NO3)2 + 2NO2 + 2H2O) given that the rate constant k is 2.31 x 10^-6 mol L^-1 s^-1 at 25°C and the rate constant increases to 3.81 x 10^-5 mol L^-1 s^-1 at 45°C.

asked Feb 4 in ElectroChemistry by ClairWaite7 (1.8k points)

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