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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 DeanneMack98 (2.1k points)

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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 LeonelSiede (1.9k points)

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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 TiffaniWymar (1.6k points)

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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 DeboraMccomb (1.9k points)

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1 answer 84 views

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 AnjaAbt20068 (2.0k points)

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1 answer 89 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 HoraceT7712 (2.0k points)

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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 NicholeBueno (1.8k points)

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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 JoelPrentice (1.4k points)

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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 LarhondaKeel (1.6k points)

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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 MAQShelton1 (1.7k points)

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1 answer 57 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 Latonya89F54 (2.2k points)

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1 answer 83 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 Maura45O7086 (2.5k points)

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1 answer 124 views

Calculate the corrosion potential of a nickel metal electrode in a 0.1 M NaCl solution with a pH of 7.2, given that the standard electrode potential for the Ni2+/Ni redox reaction is -0.25 V vs. the standard hydrogen electrode.

asked Jan 23 in ElectroChemistry by Annett65L392 (2.1k points)

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Calculate the corrosion potential of a copper metal electrode in a solution containing 0.1M CuSO4 and 0.5M H2SO4 at 298K, given that the standard electrode potential of the Cu2+/Cu electrode is +0.34V and a hydrogen electrode is used as the reference electrode.

asked Jan 23 in ElectroChemistry by GreggTimperl (2.4k points)

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1 answer 68 views

Calculate the corrosion potential of a copper metal electrode in a 0.1 M CuSO4 solution at 25°C, given that the standard reduction potential of Cu2+/Cu is +0.34 V.

asked Jan 23 in ElectroChemistry by JackQ7308746 (2.0k points)

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Calculate the corrosion potential of a copper electrode that is coupled with a silver electrode in a 0.010 M silver nitrate solution at 25°C. Given that the standard reduction potential for Ag+ + e- → Ag is +0.80V and for Cu2+ + 2e- → Cu is +0.34V. What is the potential of the copper electrode with respect to the standard hydrogen electrode?

asked Jan 23 in ElectroChemistry by SuzannaRayfo (1.8k points)

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Calculate the corrosion potential of a copper electrode immersed in a 1 M CuSO4 solution in contact with a silver electrode immersed in a 1 M AgNO3 solution. Given that the standard reduction potentials of Cu2+/Cu and Ag+/Ag are +0.34 V and +0.80 V, respectively. Determine which electrode will corrode and which electrode will act as a cathode in the galvanic cell.

asked Jan 23 in ElectroChemistry by HoraceT7712 (2.0k points)

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1 answer 89 views

Calculate the corrosion potential of a copper electrode immersed in a 0.10 M solution of copper(II) sulfate at 25°C, given that the standard reduction potential of Cu2+/Cu is +0.34 V and the pH of the solution is 4.5.

asked Jan 23 in ElectroChemistry by JuliannSfd66 (2.0k points)

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1 answer 85 views

Calculate the corrosion potential for an iron electrode in a galvanic couple with a standard hydrogen electrode at 25°C if the concentration of Fe2+ ion is 0.05 M and pH is 7.

asked Jan 23 in ElectroChemistry by TerrieGaffne (1.6k points)

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1 answer 84 views

Calculate the corrosion potential for a pure iron (Fe) electrode in a 1 M HCl solution at 25°C, given that the standard reduction potential of Fe in acidic solution is -0.44 V.

asked Jan 23 in ElectroChemistry by AnibalX1615 (2.1k points)

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