Recent questions in ElectroChemistry

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A student is given a lead-acid battery, which has a standard reduction potential of -0.356 V. The battery is undergoing a reaction where Pb(s) + SO4^2-(aq) -> PbSO4(s) + 2e^-. If the concentration of PbSO4 in the anode compartment is 1.15 M and the concentration of PbSO4 in the cathode compartment is 0.55 M, what is the power output of the battery, assuming it has a current of 1.25 A?

asked Jan 22 in ElectroChemistry by Francine68A5 (430 points)

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A student is given a galvanic cell that has a copper electrode and a silver electrode. The concentration of copper ions in the solution surrounding the copper electrode is 1.0 M, and the silver electrode is submerged in a solution of AgNO3 with a concentration of 0.1 M. The cell temperature is 25°C. Calculate the resistance of the electrochemical cell given that the cell is at equilibrium and the cell potential is measured to be 0.46 volts.

asked Jan 22 in ElectroChemistry by ElijahGlaspi (510 points)

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A student is given a galvanic cell consisting of a zinc electrode and a copper electrode. If the concentration of zinc ions in the zinc half-cell is 0.1 M and the concentration of copper ions in the copper half-cell is 1.0 M, what is the corrosion potential of the zinc electrode at standard conditions? (Assume that the standard electrode potential of copper is +0.34 V and that of zinc is -0.76 V.)

asked Jan 22 in ElectroChemistry by KatlynCantam (310 points)

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A student is given a concentration of 0.1 M of CuSO4 and 0.2 M of AgNO3, and is asked to calculate the total resistance of an electrochemical cell with electrodes made of these two solutions separated by a salt bridge. The standard reduction potentials for Cu and Ag are +0.34 V and +0.80 V, respectively. Calculate the total resistance of the cell at 25°C assuming that the cell has a thickness of 1 cm and a cross-sectional area of 10 cm².

asked Jan 22 in ElectroChemistry by KatherinDenn (730 points)

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1 answer 5 views

A student is designing an electrochemical cell using zinc and copper electrodes. The student wants to know the current density (in A/cm²) when the cell operates at a voltage of 1.5 V and a temperature of 25°C. The area of the zinc electrode is 10 cm², and the area of the copper electrode is 5 cm². Assuming a 2:1 ratio for the transfer of electrons between the two electrodes, calculate the current density in the cell.

asked Jan 22 in ElectroChemistry by MagdaAcuna34 (650 points)

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1 answer 84 views

A student conducted an experiment to calculate the Faraday constant using a silver-copper voltaic cell. The masses of the copper and silver electrodes were 4.023g and 4.721g respectively. The cell was run for 782 seconds at a constant current of 0.250A. Calculate the value of the Faraday constant for this experiment.

asked Jan 22 in ElectroChemistry by AngleaLongwe (180 points)

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1 answer 78 views

A student conducted an electrolysis experiment using a current of 2 amperes for 30 minutes with a copper sulfate solution. What is the mass of copper deposited on the cathode? The atomic weight of copper is 63.546 g/mol and the Faraday constant is 96,485 C/mol.

asked Jan 22 in ElectroChemistry by WilliamsRpu6 (390 points)

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1 answer 49 views

A student conducted an electrochemical reaction using a copper electrode to reduce a solution containing Ag+ ions. The standard reduction potential for Ag+ is 0.80 V and the standard reduction potential for Cu2+ is 0.34 V. The student measured the cell potential to be 0.62 V. Calculate the overpotential of the reaction and determine if the reduction of Ag+ occurs spontaneously.

asked Jan 22 in ElectroChemistry by VictorTuq802 (410 points)

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A steel pipeline is being used to transport a chemical mixture containing sulfuric acid. Given the concentration of sulfuric acid in the mixture and the surface area of the pipeline, calculate the corrosion rate of the steel pipeline in millimeters per year. Show your calculation and explain the significance of the result.

asked Jan 22 in ElectroChemistry by BHIJacelyn93 (390 points)

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1 answer 5 views

A steel pipe is in contact with a copper pipe in a galvanic couple, with the steel pipe acting as the anode. The corrosion current density of the steel pipe in the couple is 0.008 mA/cm². Determine the rate of corrosion of the steel pipe, assuming that the density of steel is 7.8 g/cm³ and the thickness of the pipe is 2.5 mm. Also, calculate the time taken for the pipe to corrode completely, assuming an initial mass of 5 kg.

asked Jan 22 in ElectroChemistry by ChristaJerse (350 points)

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1 answer 40 views

A steel pipe is connected to a copper pipe in a galvanic corrosion couple where the electrolyte is seawater. The corrosion current density of the steel pipe is 3.2 mA/cm2. If the surface area of the steel pipe is 5 cm2, calculate the total amount of charge transferred per hour. Also, calculate the weight loss of the steel pipe per year due to galvanic corrosion, assuming the density of steel is 7.85 g/cm3.

asked Jan 22 in ElectroChemistry by KristoferS23 (550 points)

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1 answer 55 views

A solution of NaCl was electrolyzed using a current of 2.0 A for 30 minutes. If 0.20 grams of NaCl was consumed in the process, what is the value of the Faraday constant?

asked Jan 22 in ElectroChemistry by OlivePidgeon (410 points)

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1 answer 53 views

A solution of 0.1 M AgNO3 was electrolyzed using a current of 0.5 A for 150 seconds. If 0.15 g of silver was deposited, what is the value of the Faraday constant?

asked Jan 22 in ElectroChemistry by CornellSumme (390 points)

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1 answer 42 views

A solution contains 0.1 M of an unknown ion X. The electrode potential of this ion X is measured to be +0.60 V versus the standard hydrogen electrode (SHE). Calculate the concentration of ion X in the solution using electrochemical methods.

asked Jan 22 in ElectroChemistry by DinaTrimm852 (530 points)

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1 answer 65 views

A solution contains 0.05 mol of Cu^2+ ions. If a current of 0.5 A is passed through this solution for 15 minutes, what is the value of the Faraday constant?

asked Jan 22 in ElectroChemistry by LuellaLind54 (250 points)

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1 answer 5 views

A solution contains 0.05 M AgNO3 and 0.10 M KCl. A silver electrode is dipped in the solution and a potential of 0.53 V is measured against a standard hydrogen electrode. Calculate the concentration of Ag+ ions in the solution.

asked Jan 22 in ElectroChemistry by AnastasiaDwi (370 points)

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1 answer 65 views

A solution containing 0.5 moles of potassium dichromate was electrolyzed with a current of 1.5 Amperes for 30 minutes. During the process, the final volume of the solution was found to be 250 mL. Calculate the value of the Faraday constant using this information.

asked Jan 22 in ElectroChemistry by RileyBethune (430 points)

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1 answer 6 views

A piece of zinc metal is placed in a beaker containing an acidic solution, while a copper electrode is also placed in the same solution. The copper electrode is connected to the positive terminal of a voltmeter, while the zinc electrode is connected to the negative terminal of the voltmeter. If the measured potential between the two electrodes is -0.76 V, what is the corrosion potential of the zinc electrode?

asked Jan 22 in ElectroChemistry by StaciStrub6 (450 points)

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A metal rod of 3 cm diameter and 20 cm length is placed in a solution of hydrochloric acid with a pH of 2 at 25°C. The metal has a critical pitting temperature of 40°C and a standard electrode potential of -0.44V. Assuming that the rod is polarized to a potential of -0.50V, what is the corrosion current density (in mA/cm²) of the metal in the given environment?

asked Jan 22 in ElectroChemistry by JackieEarly7 (510 points)

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A metal rod made of iron is coupled with a zinc rod in an aqueous medium. If the corrosion potential of the iron rod is -0.44 V and that of the zinc rod is -0.76 V, calculate the corrosion current density of the iron rod when coupled with the zinc rod at 25°C. The polarization resistance of the iron rod is 880 Ωcm².

asked Jan 22 in ElectroChemistry by SashaTellez5 (370 points)

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