Recent questions in Chemistry

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Calculate the dipole moment of carbon dioxide molecule and determine its polarity.

asked Jan 23 in Chemical bonding by ClariceMcQui (430 points)

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1 answer 12 views

Calculate the dipole moment of carbon dioxide (CO2) molecule using ab initio calculations at the HF/6-311+G(d,p) level of theory. How does it compare to the experimentally measured dipole moment value? Explain the reason for any differences observed.

asked Jan 23 in Computational Chemistry by Brian0571409 (420 points)

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1 answer 48 views

Calculate the density of solid sodium chloride given that its mass is 5.50 g and its volume is 2.50 cm³.

asked Jan 23 in Inorganic Chemistry by EdgardoSchon (220 points)

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1 answer 64 views

Calculate the density of barium sulfate ($\text{BaSO}_{4}$) with a molecular weight of 233.39 g/mol, assuming a sample with a mass of 5 g occupies a volume of 3 mL.

asked Jan 23 in Inorganic Chemistry by LynMairinger (310 points)

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1 answer 65 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 JacksonBoxal (230 points)

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1 answer 69 views

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 EvonneSeiler (370 points)

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1 answer 50 views

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 CandiceDurbi (590 points)

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1 answer 55 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 AbigailWight (510 points)

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1 answer 48 views

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 JannieBrindl (370 points)

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1 answer 48 views

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 LeonelPiddin (250 points)

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1 answer 53 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 CristineHill (250 points)

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1 answer 50 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 AndresReaves (460 points)

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1 answer 57 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 SheriFkw4940 (270 points)

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1 answer 58 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 MandyFinley (190 points)

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1 answer 68 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 Mira74D62054 (330 points)

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1 answer 58 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 FranceDease7 (50 points)

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1 answer 64 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 TeresaCulpep (330 points)

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1 answer 58 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 Nathan39B173 (210 points)

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1 answer 75 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 SueFcg023218 (210 points)

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1 answer 37 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 KarinGreer69 (490 points)

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