Recent questions in ElectroChemistry

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Calculate the resistance of an electrochemical cell given the following parameters: - The cell has a total area of 50 cm² and a separation between the electrodes of 2 cm.- The electrolyte solution has a conductivity of 2.5 × 10⁻⁴ S/cm and a temperature of 25°C.- The electrode on the left side of the cell is made of platinum and has a surface area of 25 cm². The electrode on the right side is made of silver and has a surface area of 25 cm².- The distance between each electrode and the solution is 0.5 cm.

asked Feb 3 in ElectroChemistry by JosetteSarto (2.0k points)

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1 answer 86 views

Calculate the resistance of an electrochemical cell constructed by using a copper electrode in a 1M copper (II) sulfate solution and a zinc electrode in a 1M zinc sulfate solution. The measured potential difference of the cell is 1.45 volts. The area of each electrode is 10cm² and the length of wire connecting the electrodes is 30cm with a cross-sectional area of 1 mm². The conductivity of copper (II) sulfate and zinc sulfate solutions at the given concentration is 98.3% and 89.9% respectively. What is the resistance (in ohms) of the electrochemical cell?

asked Feb 3 in ElectroChemistry by JeremyCanady (2.1k points)

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1 answer 89 views

Calculate the resistance of a electrochemical cell at 25°C if the standard reduction potential of the anode is -1.36 V and the standard reduction potential of the cathode is +0.40 V. The solution contains 0.1 M CuSO4 and 0.01 M ZnSO4. The distance between the two electrodes is 5 cm and the cross-sectional area of each electrode is 2.5 cm².

asked Feb 3 in ElectroChemistry by TarenSalmond (1.8k points)

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1 answer 72 views

Calculate the rate of the electrochemical reaction when a current of 2.5 A is passed through a solution of copper sulphate for 2 hours, and 4 g of copper is formed at the cathode. The atomic weight of copper is 63.5 g/mol.

asked Feb 3 in ElectroChemistry by ClevelandHaw (2.4k points)

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1 answer 59 views

Calculate the rate of the electrochemical reaction that takes place in the following electrolytic cell:Cu(s) | Cu2+(aq, 0.050 M) || Ag+(aq, 0.010 M) | Ag(s)Given that the current density is 0.500 A/m2 and the Faraday constant is 96,485 C/mol. The reduction potential of Cu2+(aq) + 2e- → Cu(s) is +0.34 V, and the reduction potential of Ag+(aq) + e- → Ag(s) is +0.80 V. Assume the temperature is 25°C and one-unit charge is exchanged.

asked Feb 3 in ElectroChemistry by FelixTolmer3 (1.9k points)

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1 answer 73 views

Calculate the rate of electroplating of copper on a metallic surface at a current of 2.5 amperes for a duration of 3 hours using a copper nitrate solution with a concentration of 0.2 M. Given that the standard potential of the reduction reaction of Cu2+ to Cu is +0.34 V and the charge of one mole of electrons is 96500 C/mol.

asked Feb 3 in ElectroChemistry by RudyMms5536 (1.8k points)

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1 answer 68 views

Calculate the power output of an electrochemical cell that uses a cathode made of silver metal immersed in a solution containing silver ions with a concentration of 0.05 M and an anode made of zinc metal immersed in a solution containing zinc ions with a concentration of 0.1 M. The temperature of the solutions is 298 K and the cell operates at a current of 0.5 A.

asked Feb 3 in ElectroChemistry by EdytheEwk100 (2.6k points)

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1 answer 67 views

Calculate the power output of a galvanic cell having a standard potential of +0.76V and a current of 0.5A flowing through it. The cell consists of a zinc electrode and a copper electrode connected by a salt bridge and the concentration of the electrolyte is 1.0M. Given that the Faraday constant is 96487 C/mol and the temperature is 298K.

asked Feb 3 in ElectroChemistry by EvieOconnor (2.3k points)

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1 answer 58 views

Calculate the power output of a galvanic cell given that the cell potential is 1.8 V and the current passing through the circuit is 2.5 A. The electrochemical reaction taking place in the cell is the oxidation of Zinc and reduction of Copper. The standard reduction potentials are +0.76 V for copper and -0.76 V for zinc. The concentration of Zinc ions is 1.0 M whereas Copper ions concentration is 0.1 M. Determine the power output of the cell.

asked Feb 3 in ElectroChemistry by ElenaBriscoe (2.1k points)

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1 answer 80 views

Calculate the power output of a Galvanic cell consisting of a standard hydrogen electrode and a standard copper electrode at 298 K when the concentration of copper ions in the cathode half-cell is 0.1 M and hydrogen gas pressure in the anode half-cell is at 1 bar. The standard reduction potentials for the hydrogen and copper half-reactions are +0.0 V and +0.34 V, respectively.

asked Feb 3 in ElectroChemistry by VickeyBatema (1.9k points)

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1 answer 106 views

Calculate the power output for a Zinc-Copper electrochemical cell operating at standard conditions with a Zinc electrode that measures 10 cm by 12 cm and a Copper electrode that measures 8 cm by 10 cm. The current flowing through the circuit is 0.5 A. The standard reduction potentials for the half-reactions are +0.76 V for Cu2+/Cu and -0.76 V for Zn2+/Zn.

asked Feb 3 in ElectroChemistry by StarMayo945 (1.8k points)

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1 answer 78 views

Calculate the potential difference between two silver electrodes that are placed into a solution containing 0.1M of AgNO3 and a current of 2.5 A is passed through the cell. The polarization caused by the passage of current through the cell is found to be 0.2 V. Given that the standard reduction potential of Ag+ to Ag is 0.80 V, calculate the equilibrium potential of the cell.

asked Feb 3 in ElectroChemistry by CatherineMcc (2.5k points)

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1 answer 92 views

Calculate the polarization that occurs in an electrochemical cell when a current of 2 A flows through it for 10 minutes. The electrode area is 25 cm², and the current efficiency is 95%. The activation energy is 80 kJ/mol, and the reaction quotient is 2.5 x 10⁻⁵. The temperature of the cell is 25°C. Find the polarization resistance and the total polarization of the cell.

asked Feb 3 in ElectroChemistry by AleciaAlleyn (1.5k points)

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1 answer 86 views

Calculate the polarization resistance of a copper electrode in a 0.1 M copper sulfate solution at 25°C, given that the current density is 10 mA/cm² and the exchange current density is 0.1 mA/cm². The Tafel slope is 30 mV/decade.

asked Feb 3 in ElectroChemistry by HeidiElmslie (1.8k points)

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1 answer 124 views

Calculate the polarization potential in an electrochemical cell if the concentration of zinc ions in the anode compartment is 0.5 M, the concentration of copper(II) ions in the cathode compartment is 1.0 M, and the voltage of the cell is 1.1 V. The standard reduction potential of copper(II) ions is +0.34 V and the standard reduction potential of zinc ions is -0.76 V.

asked Feb 3 in ElectroChemistry by HesterLoyau3 (2.1k points)

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1 answer 85 views

Calculate the polarization of a copper-silver galvanic cell in which the concentration of copper ions is 0.5 M, the concentration of silver ions is 0.1 M, and the cell is operating at a temperature of 25°C. The potential difference of the cell is measured to be 0.75 V.

asked Feb 3 in ElectroChemistry by VioletteM27 (2.1k points)

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1 answer 46 views

Calculate the polarization of a copper electrode immersed in a 0.1 M CuSO4 solution at 25°C when it is coupled to a hydrogen electrode with a hydrogen pressure of 1 atm. Given that the standard reduction potential of Cu2+|Cu electrode is 0.34 V and the standard reduction potential of H+|H2 electrode is 0 V at 25°C.

asked Feb 3 in ElectroChemistry by JadaMeece33 (1.6k points)

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1 answer 77 views

Calculate the polarization of a cell having an anode made of copper metal immersed in a 1.0 M Cu(NO3)2 solution and a cathode made of silver metal in a 1.0 M AgNO3 solution. Given that the potential of the copper electrode is -0.34 V and that of the silver electrode is 0.80 V. Also, assume that the current density is 0.1 A/cm² and that the temperature is 298 K.

asked Feb 3 in ElectroChemistry by JaimeFuqua07 (2.0k points)

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1 answer 68 views

Calculate the polarization in an electrochemical cell consisting of a zinc electrode and a copper electrode. The electrode potentials of zinc and copper are -0.76 V and +0.34 V, respectively. The resistance of the electrolyte solution between the electrodes is 10 ohms, and the current flowing through the cell is 0.5 A.

asked Feb 3 in ElectroChemistry by ClydeC545764 (2.2k points)

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1 answer 83 views

Calculate the overpotential of an electrochemical cell where Zinc metal is used as an anode and Copper metal as a cathode. The concentration of Zinc ions in the half-cell is 1 M and Copper ions in the half-cell is 0.1 M. The temperature of the system is 25°C. (Given: Standard Reduction Potentials - Zn²⁺ + 2e⁻ → Zn(s) = -0.76 V and Cu²⁺ + 2e⁻ → Cu(s) = +0.34 V)

asked Feb 3 in ElectroChemistry by jozzpfdeimmyapm (2.0k points)

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