Recent questions in ElectroChemistry

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Calculate the equilibrium constant (K) for the reaction between copper and silver ions in a galvanic cell at room temperature (25°C), given the following half-reactions and their respective reduction potentials:Cu2+ (aq) + 2e- → Cu (s) E°red = +0.34 VAg+ (aq) + e- → Ag (s) E°red = +0.80 VAlso, if the cell is constructed with a copper electrode and a silver electrode, which electrode will be the cathode and which will be the anode?

asked Jan 23 in ElectroChemistry by LakeishaA172 (500 points)

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Calculate the equilibrium constant (K) for the electrochemical reaction: Mg(s) + 2 Ag+(aq) → Mg2+(aq) + 2 Ag(s) Given that the standard reduction potentials for Ag+ and Mg2+ are +0.80 V and -2.37 V, respectively. The concentration of Ag+ is 0.020 M and the concentration of Mg2+ is 0.080 M.

asked Jan 23 in ElectroChemistry by MarshaReiss (430 points)

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Calculate the efficiency of an electrochemical cell with a standard potential of +0.80 V if the cell potential under operating conditions is +0.60 V and the current passing through the cell is 2.5 A.

asked Jan 23 in ElectroChemistry by JaquelineGel (450 points)

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1 answer 53 views

Calculate the current density of an electrochemical cell where a nickel electrode is oxidized to form nickel (II) ions, while a copper electrode is reduced by the nickel (II) ions. The cell has a voltage of 0.65 volts and a resistance of 50 ohms. The surface area of the nickel electrode is 10 cm² while that of the copper electrode is 15 cm². The current density of the electrochemical cell is expressed in A/cm².

asked Jan 23 in ElectroChemistry by DollySelig78 (410 points)

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Calculate the current density in an electrochemical cell if a current of 2.5 A is passed through a copper electrode with a surface area of 25 cm² and a silver electrode with a surface area of 10 cm² for 3 hours. The half-cell potentials of copper and silver electrodes are +0.34 V and +0.80 V, respectively, and the molar concentrations of copper and silver ions in the electrolyte are 0.5 M and 1 M, respectively.

asked Jan 23 in ElectroChemistry by ZVWShalanda (590 points)

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Calculate the current density in an electrochemical cell if a current of 2.5 A is passed through a cell containing 0.150 L of a 0.250 M solution of CuSO4 for 2.00 hours. The cathodic half-reaction is Cu2+ + 2e- → Cu and the anodic half-reaction is Zn → Zn2+ + 2e-. The cell has a standard potential of 1.10 V at 298 K. What is the current density of the cell?

asked Jan 23 in ElectroChemistry by PIGPoppy325 (1.0k points)

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1 answer 45 views

Calculate the corrosion rate of iron (Fe) in a galvanic couple with copper (Cu), given that the area of the iron electrode is 8 cm² and the current density is 0.6 mA/cm². The standard electrode potential of iron is -0.44 V and that of copper is +0.34 V.

asked Jan 23 in ElectroChemistry by OnaKee41409 (390 points)

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Calculate the corrosion rate of an iron rod with a surface area of 20 cm² that is connected to a copper plate with a surface area of 25 cm², immersed in a solution of 0.5 M copper sulfate, given that the measured current is 0.2 A.

asked Jan 23 in ElectroChemistry by ChiKramer817 (350 points)

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Calculate the corrosion rate of a steel rod when it is placed in a galvanic coupling with a copper strip at 25°C. The initial weight of the steel rod was 28.6 g and it lost 0.48 g in weight after 24 hours of exposure. The area of the steel rod in contact with the electrolyte solution is 3.14 cm² and the electrode potential of the copper strip is +0.34V while the electrode potential of the steel rod is -0.44V. Using Faraday’s law of electrolysis, determine the corrosion rate of the steel rod in mmpy (mils per year).

asked Jan 23 in ElectroChemistry by MargaritaL74 (250 points)

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1 answer 44 views

Calculate the corrosion rate of a copper wire of diameter 0.5 cm and length 20 cm when immersed in a solution containing 1M HCl for 24 hours. The initial and final weights of the wire were 6.0 g and 5.6 g, respectively. The density of copper is 8.96 g/cm³. What is the corrosion rate of the copper wire in mm/year?

asked Jan 23 in ElectroChemistry by DeboraPrenti (250 points)

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1 answer 48 views

Calculate the corrosion rate of a copper metal when it is placed in a galvanic couple with zinc metal. The potential difference between the two metals is measured to be 1.5 V and the surface area of the copper metal is 2 cm². The density of copper is 8.96 g/cm³ and its atomic weight is 63.546 g/mol. The atomic weight of zinc is 65.38 g/mol and its density is 7.14 g/cm³. At constant temperature and pressure, assume that the Faraday constant is 96,485 Coulombs/mol and that one mole of electrons is equivalent to one Faraday.

asked Jan 23 in ElectroChemistry by DaltonMcDone (530 points)

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1 answer 41 views

Calculate the corrosion rate of a 5mm thick copper wire that is exposed to a saline solution of 20% NaCl at a temperature of 25°C, knowing that the wire has lost 3 grams of mass in 10 days of exposure.

asked Jan 23 in ElectroChemistry by LazaroR32061 (290 points)

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Calculate the corrosion potential of iron in an acidic environment with a pH of 3.5, given that the half-reaction for the reduction of Fe3+ to Fe2+ is Fe3+ + e- → Fe2+ and the standard reduction potential (E°) for this half-reaction is +0.771 V.

asked Jan 23 in ElectroChemistry by MargieSelph6 (470 points)

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1 answer 55 views

Calculate the corrosion potential of iron (Fe) in a 1 M solution of hydrochloric acid (HCl) at 25°C, given that the standard reduction potential of Fe is -0.44 V and the standard reduction potential of HCl is 1.36 V. What is the likelihood of iron corroding in this environment?

asked Jan 23 in ElectroChemistry by KoryLongstaf (330 points)

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1 answer 46 views

Calculate the corrosion potential of iron (Fe) in a 0.1 M HCl solution at 25°C, given that the standard electrode potential for the Fe2+/Fe redox couple is -0.44 V and the standard hydrogen electrode potential at the same temperature and pressure is 0 V. What is the likelihood of iron corrosion in this environment?

asked Jan 23 in ElectroChemistry by KristiAinsli (450 points)

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1 answer 43 views

Calculate the corrosion potential of copper in seawater environment having a pH of 8.2 and a temperature of 25°C given that the standard hydrogen electrode potential is -0.76 V and the concentration of copper ions in seawater is 2.5 x 10^-5 M.

asked Jan 23 in ElectroChemistry by ElaneLavarac (590 points)

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1 answer 47 views

Calculate the corrosion potential of copper in a galvanic couple with a standard hydrogen electrode at 298 K, given that the standard electrode potential of copper is +0.34 V and the standard electrode potential of hydrogen is 0 V.

asked Jan 23 in ElectroChemistry by Margarita30G (490 points)

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1 answer 59 views

Calculate the corrosion potential of a zinc-copper galvanic couple in which the zinc electrode has a concentration of 0.1 M and the copper electrode has a concentration of 0.01 M. The standard reduction potentials for Zn2+/Zn and Cu2+/Cu are -0.76 V and +0.34 V, respectively.

asked Jan 23 in ElectroChemistry by Winston54817 (550 points)

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1 answer 27 views

Calculate the corrosion potential of a silver metal in a solution containing 0.1 M silver nitrate and 1 M nitric acid given that the standard reduction potential of the Ag⁺/Ag couple is +0.80 V and the standard reduction potential of the NO₃⁻/NO₂⁻ couple is +0.96 V.

asked Jan 23 in ElectroChemistry by BraydenPlume (510 points)

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1 answer 48 views

Calculate the corrosion potential of a pure copper metal electrode immersed in a 0.1 M solution of CuSO4 at 298 K, given that the standard electrode potential of Cu2+/Cu is +0.34 V and the standard potential of the hydrogen electrode is 0 V. Assume that activity coefficients for copper ions and sulfate ions are equal to 1.0 in the solution. What is the likelihood that this copper electrode will corrode in this given environment?

asked Jan 23 in ElectroChemistry by KiaLarios92 (380 points)

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