Recent questions in ElectroChemistry

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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 ZacheryWilli (250 points)

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1 answer 47 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 KellyMuirden (550 points)

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A zinc rod is being placed in a solution containing 0.1 M of copper (II) ions. Calculate the corrosion potential of the zinc rod in a galvanic couple with a standard hydrogen electrode at 25°C.

asked Jan 22 in ElectroChemistry by DemetriaOhma (350 points)

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A zinc electrode was kept in a 0.1 M ZnSO4(aq) solution, and a copper electrode was kept in a 0.1 M CuSO4(aq) solution. When 1500 C of electricity was passed through the cell, how many grams of copper were deposited on the cathode? (Assume 100 % efficiency and the Faraday constant is 96500 C/mol)

asked Jan 22 in ElectroChemistry by GeriFarquhar (350 points)

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1 answer 42 views

A zinc electrode is immersed in a 1.0 M ZnSO4 solution and connected to a platinum electrode that is immersed in a 1.0 M CuSO4 solution. If the measured potential difference of the cell is 1.10 V at 25 °C, what is the polarization of the cell?

asked Jan 22 in ElectroChemistry by KatherineBur (570 points)

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1 answer 36 views

A zinc electrode is connected to a copper electrode by a wire in a beaker that has a solution of 0.1 M CuSO4 and 0.1 M ZnSO4. The initial reduction potential of the copper electrode is +0.34 V, and the initial oxidation potential of zinc is –0.76 V. What is the potential difference between the two electrodes at 298 K, and what is the rate of the electrochemical reaction when the cell operates at a current of 2.50 A?

asked Jan 22 in ElectroChemistry by LawrenceDyal (530 points)

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A voltaic cell consists of a standard hydrogen electrode and a copper electrode in a solution of copper(II) sulfate. The measured cell potential is 0.78 V at 25°C. If the concentration of copper(II) sulfate is 0.1 M, what is the resistance of the electrochemical cell?

asked Jan 22 in ElectroChemistry by BessieBrobst (410 points)

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1 answer 47 views

A student wishes to determine the power output of an electrochemical cell that utilizes a half-reaction of copper oxide reducing to copper and a half-reaction of zinc oxidizing to zinc ions. The initial concentrations of the copper and zinc ions in the cell are 1.00 M and 0.10 M, respectively. The cell operates for 60 minutes at a constant rate of 0.200 A. Given that the standard cell potential is 1.10 V, calculate the power output of the electrochemical cell.

asked Jan 22 in ElectroChemistry by EmmaLeist635 (400 points)

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1 answer 42 views

A student wants to find out the cell potential of a voltaic cell made up of a nickel electrode and an iron electrode. The nickel electrode is in a 0.1 M nickel (II) sulfate solution, and the iron electrode is in a 0.1 M iron (II) sulfate solution. What is the cell potential of this voltaic cell at standard conditions (25°C and 1 atm of pressure) given the standard reduction potentials for Ni2+/Ni and Fe2+/Fe are -0.25 V and -0.44 V, respectively?

asked Jan 22 in ElectroChemistry by EdmundGopink (230 points)

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1 answer 49 views

A student wants to electroplate a piece of copper with silver in an electrochemical cell. If a current of 0.5 A is passed through the cell for 30 minutes, what mass of silver will be deposited on the copper piece? The atomic mass of silver is 107.87 g/mol and the faraday constant is 96,485 C/mol.

asked Jan 22 in ElectroChemistry by CandraDawbin (530 points)

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1 answer 7 views

A student wants to electroplate a nickel wire with copper. The student has 1 g of copper sulfate and a 2 M solution of sulfuric acid. The wire has a surface area of 3 cm², and the desired copper thickness on the wire is 0.025 cm. How long should the student electroplate the wire with a current of 1.5 A to achieve the desired thickness of copper? Calculate the current density in the electrochemical cell.

asked Jan 22 in ElectroChemistry by EssieHimes15 (350 points)

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1 answer 47 views

A student wants to determine the power output of a galvanic cell containing a zinc electrode and a copper electrode. The zinc electrode has a surface area of 20 cm² and is coated with a layer of zinc which weighs 0.5 grams. The copper electrode has a surface area of 15 cm² and is coated with a layer of copper that weighs 0.4 grams. The cell operates at standard conditions (25°C and 1 atm), and the electrolyte is a solution of 1 M copper sulfate and 1 M zinc sulfate. Calculate the power output of the electrochemical cell.

asked Jan 22 in ElectroChemistry by Kaley34M2669 (430 points)

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1 answer 6 views

A student wants to determine the polarization in an electrochemical cell where the anode is made of zinc and the cathode is made of copper. The electrolyte used is CuSO4. The current through the cell is 0.5 A and the measured potential difference is 1.5 V. What is the polarization of this electrochemical cell?

asked Jan 22 in ElectroChemistry by DrusillaDesi (450 points)

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1 answer 5 views

A student wants to determine the maximum voltage and power output of a primary cell that consists of a zinc electrode in 1M Zn(NO3)2 solution and a silver electrode in 1M AgNO3 solution. The student knows the standard reduction potentials of Zn2+/Zn and Ag+/Ag to be -0.76V and +0.80V, respectively. Assuming the cell operates under standard conditions at 298K, what is the maximum voltage that the cell can generate and the maximum power output it can deliver?

asked Jan 22 in ElectroChemistry by FSLBrigida46 (470 points)

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1 answer 54 views

A student wants to determine the mass of silver (Ag) that will be deposited on the cathode when a current of 4 A passes through a solution of silver nitrate (AgNO3) for 30 minutes. What is the mass of silver that will be deposited on the cathode? (Assume a Faraday constant of 96,485 C/mol and the atomic mass of silver is 107.87 g/mol).

asked Jan 22 in ElectroChemistry by OliverY88898 (370 points)

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1 answer 48 views

A student wants to determine the concentration of silver ions (Ag+) in a solution. Using an Ag/Ag+ reference electrode, the student measures the cell potential to be +0.56 V when the solution is electrolyzed for 25 minutes at a constant current of 0.50 A. The volume of the solution is 150 mL. What is the concentration of silver ions in the solution in mol/L?

asked Jan 22 in ElectroChemistry by Connie104727 (470 points)

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1 answer 7 views

A student wants to calculate the rate of an electrochemical reaction. They know that the concentration of the anodic reactant is 0.01 M and that the cathodic reactant is at a concentration of 0.02 M. The student also knows that the cell potential is 1.23 V, and that the Faraday's constant is 96485 C/mol. The reaction is:Fe(s) + Cu2+(aq) → Fe2+(aq) + Cu(s)What is the rate of the reaction in mol/s at standard conditions (25°C and 1 atm)?

asked Jan 22 in ElectroChemistry by Korey4583669 (230 points)

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1 answer 49 views

A student wants to calculate the efficiency of an electrochemical cell with a standard potential of -0.74 volts. The cell is set up with a copper electrode immersed in a solution of copper(II) sulfate and a silver electrode immersed in a solution of silver nitrate, connected by a salt bridge. The student measures a current of 0.5 amperes flowing through the cell for a duration of 60 minutes. Calculate the efficiency of the electrochemical cell in terms of the amount of reactants consumed and the amount of product formed.

asked Jan 22 in ElectroChemistry by MaximilianFi (370 points)

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1 answer 6 views

A student wants to calculate the corrosion rate of a zinc electrode in contact with a copper electrode, with a measured current of 0.5 amperes and a surface area of 2 cm². Given that the standard reduction potentials for copper and zinc electrodes are +0.34 V and -0.76 V, respectively, what is the corrosion rate of the zinc electrode in millimeters per year? (Assume a density of 7.14 g/cm³ for zinc and a Faraday constant of 96,500 coulombs per mole).

asked Jan 22 in ElectroChemistry by ShermanGregs (370 points)

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1 answer 47 views

A student wants to calculate the amount of copper deposited on the cathode during the electrolysis of a copper (II) sulfate solution. If 2.5 A of current is passed through the cell for 10 minutes, what is the mass of copper that is deposited on the cathode? (Assume the atomic weight of copper is 63.55 g/mol and the Faraday constant is 96,485 C/mol).

asked Jan 22 in ElectroChemistry by ArianneDuhig (610 points)

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