Recent questions in ElectroChemistry

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Here's a precise problem for the student to solve:A galvanic cell is constructed with a zinc electrode and a copper electrode in two separate solutions, connected by a salt bridge. The zinc electrode has a surface area of 4 cm² and the copper electrode has a surface area of 8 cm². The concentration of zinc ion solution is 0.1 M and the copper ion solution is 0.01 M. The temperature of the solutions is 25°C. Calculate the resistance of the electrochemical cell.

asked 20 hours ago in ElectroChemistry by JerilynGeake (310 points)

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Here is a question for a chemistry student to solve in the subtopic Calculation of current density in an electrochemical cell: What is the current density (in amperes per square meter) in a zinc-copper galvanic cell, given that the mass of zinc electrode is 10 g and the rate of zinc dissolution is 0.1 g/min, the area of copper electrode is 5 cm², and the potential difference between the electrodes is 1.5 V?

asked 20 hours ago in ElectroChemistry by BarrettVep43 (450 points)

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1 answer 40 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 20 hours ago in ElectroChemistry by LourdesZimpe (490 points)

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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 21 hours ago in ElectroChemistry by Kaylene42T32 (450 points)

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1 answer 31 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 21 hours ago in ElectroChemistry by KAULeora045 (510 points)

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1 answer 28 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 21 hours ago in ElectroChemistry by VictorTuq802 (410 points)

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1 answer 4 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 21 hours ago in ElectroChemistry by JanetteBrewi (450 points)

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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 21 hours ago in ElectroChemistry by ClaudiaGut87 (400 points)

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1 answer 28 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 21 hours ago in ElectroChemistry by ConcettaMira (500 points)

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1 answer 22 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 21 hours ago in ElectroChemistry by AbbeyJaspriz (510 points)

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1 answer 38 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 21 hours ago in ElectroChemistry by TerrellBejah (250 points)

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1 answer 29 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 21 hours ago in ElectroChemistry by DannySantora (590 points)

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1 answer 33 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 21 hours ago in ElectroChemistry by DessieWisnie (430 points)

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1 answer 37 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 21 hours ago in ElectroChemistry by Ernestine878 (530 points)

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1 answer 30 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 21 hours ago in ElectroChemistry by IrvinBonney (370 points)

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1 answer 22 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 21 hours ago in ElectroChemistry by VivienScheff (510 points)

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1 answer 20 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 21 hours ago in ElectroChemistry by GeraldoBohm (330 points)

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1 answer 29 views

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

asked 22 hours ago in ElectroChemistry by MaxCampa199 (290 points)

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1 answer 32 views

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

asked 22 hours ago in ElectroChemistry by FranciscoRug (470 points)

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1 answer 33 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 22 hours ago in ElectroChemistry by JaimieGuerra (590 points)

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