Recent questions in ElectroChemistry

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A metal electrode immersed in a solution is used to convert a chemical reaction into an electric current. The electrode potential is measured as the voltage difference between the metal and the solution. The cathodic and anodic Tafel slopes are then calculated in order to determine the rate of the chemical reaction occurring at the electrode. Given a metal electrode immersed in a 0.1 M solution of AgNO3, the cathodic and anodic Tafel slopes are determined to be 120 mV/decade and 110 mV/decade, respectively. Calculate the exchange current density for the reaction occurring at the electro

asked Jan 22 in ElectroChemistry by ChongChadwic (410 points)

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A galvanic cell has a standard emf of 1.10 V at 298 K. If this cell runs for 25 minutes with a constant current of 0.25 A, what is the amount of energy produced in joules? (Assume the cell is operating under standard conditions.)

asked Jan 22 in ElectroChemistry by JennyCouch7 (270 points)

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1 answer 59 views

A galvanic cell consists of a standard hydrogen electrode (SHE) as the cathode and a copper electrode as the anode. The measured potential difference between the two electrodes is 1.23 V. Using Tafel analysis, calculate the anodic and cathodic Tafel slopes for the copper electrode.

asked Jan 22 in ElectroChemistry by LorenzoBarra (310 points)

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1 answer 56 views

A current of 2.5 amperes was passed through molten silver chloride for 5 hours. What mass of silver metal will be deposited? (The atomic mass of silver = 107.87 g/mol)

asked Jan 22 in ElectroChemistry by JefferySerra (590 points)

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1 answer 37 views

A copper wire is exposed to a solution containing 0.2 M NaCl. The corrosion rate of the wire is found to be 5.8 microAmp/cm². Calculate the corrosion current density of the copper wire in the given environment.

asked Jan 22 in ElectroChemistry by Connie104727 (470 points)

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1 answer 46 views

A copper rod with a surface area of 5 cm² is coupled with an iron rod with a surface area of 10 cm² to form a galvanic cell. When the circuit is closed, the current flows for 2 hours and the weight loss of the iron rod was found to be 0.58 g. Determine the corrosion rate of the iron rod in millimeters per year (mm/yr) assuming a density of 7.86 g/cm³ for the iron.

asked Jan 22 in ElectroChemistry by Staci6700611 (450 points)

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1 answer 48 views

A copper electrode is placed in a 1.0 M Cu(NO3)2 solution while a silver electrode is placed in a 1.0 M AgNO3 solution. If the cell potential is measured to be 0.74 V at standard state conditions, what is the equilibrium constant for the reaction Cu(s) + 2Ag+(aq) ⇌ Cu2+(aq) + 2Ag(s)?

asked Jan 22 in ElectroChemistry by Edward211098 (590 points)

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1 answer 5 views

A copper electrode is immersed in a 0.1M solution of CuSO4 and a zinc electrode is immersed in 0.1M solution of ZnSO4. Both the solutions are connected with a salt bridge. If the standard reduction potentials of Cu2+/Cu and Zn2+/Zn are +0.34V and -0.76 V respectively, calculate the potential difference between the two electrodes at 25°C.

asked Jan 22 in ElectroChemistry by WalterRandol (470 points)

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1 answer 67 views

A chemistry student wants to determine the Faraday constant (F) by electroplating copper on a platinum electrode using a current of 2.0 A for 10 minutes. Calculate the amount of copper deposited and use this information to determine the value of the Faraday constant.

asked Jan 22 in ElectroChemistry by NoemiBlamey (350 points)

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1 answer 82 views

A chemistry student wants to determine the concentration of copper(II) ions in a solution using electrochemical methods. The student prepares a copper electrode and a reference electrode, and sets up a cell with the copper electrode immersed in the solution and the reference electrode in the salt bridge. The standard cell potential is measured to be +0.34 V. If the student knows that the reduction of copper(II) to copper occurs at the copper electrode, what is the concentration of copper(II) ions in the solution?

asked Jan 22 in ElectroChemistry by VidaMcAlroy6 (470 points)

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1 answer 77 views

A chemistry student needs to calculate the concentration of copper(II) ions in a 250 mL solution, given that a current of 1.5 A was applied for 60 minutes to a copper electrode in contact with the solution. The initial concentration of copper(II) ions was 0.05 M, and the Faraday constant is 96,485 C/mol. What is the final concentration of copper(II) ions in the solution?

asked Jan 22 in ElectroChemistry by LeonaSpivey (550 points)

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1 answer 62 views

A chemistry student is required to determine the cathodic and anodic Tafel slopes for a reaction occurring at an electrode surface. The current density at the cathodic surface is known to be 1.8 mA/cm² and the current density at the anodic surface is known to be 1.2 mA/cm². The current potential relationship is given by the Tafel equation:log (i) = log (i0) + β_c * (E-E_c) for cathodic reactionlog (i) = log (i0) + β_a * (E-E_a) for anodic reactionWhere i is the current density, i0 is the exchange current density, β_c and β_a are the cathodic and anodic Tafel slopes respectively, E is the elect

asked Jan 22 in ElectroChemistry by TrentAdam35 (470 points)

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1 answer 57 views

A chemistry student is given the following information: A galvanic cell is set up consisting of a copper electrode in a copper (II) ion solution connected by a salt bridge to a silver electrode in a silver ion solution. The concentration of the copper (II) solution is 0.10 M and the concentration of the silver ion solution is 0.025 M. The measured potential of the cell is 0.66 V. Calculate the resistance of this electrochemical cell.

asked Jan 22 in ElectroChemistry by KarenSamson (630 points)

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1 answer 40 views

A chemistry student is asked to find the standard cell potential for the redox reaction: Mg(s) | Mg²⁺(aq, 0.1 M) || Cu²⁺(aq, 0.01 M) | Cu(s) Given that the standard potential for the reduction of Mg²⁺ is -2.37 V and for the reduction of Cu²⁺ is +0.34 V. The student should show how to calculate the cell potential and determine if the reaction will proceed spontaneously or not.

asked Jan 22 in ElectroChemistry by DarbyEastin (210 points)

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1 answer 39 views

A chemist is attempting to electroplate copper onto a steel surface using a copper sulfate solution. The standard reduction potential for this reaction is -0.34 V, but the scientist is only seeing a voltage of -0.53 V. Calculate the overpotential for this electrochemical reaction.

asked Jan 22 in ElectroChemistry by AnkeSon38062 (310 points)

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1 answer 27 views

A brass alloy electrode with an area of 5 cm² is immersed in a 0.5 M NaCl solution at 25°C. Given that the standard potential of the electrode is -0.35 V versus a standard hydrogen electrode, calculate the corrosion current density of the electrode in the given environment using Tafel extrapolation.

asked Jan 22 in ElectroChemistry by PilarTithera (390 points)

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1 answer 30 views

A battery consists of a Zinc electrode and a Copper electrode. Calculate the exchange current density at the Zinc electrode if the concentration of Zinc ion in its solution is 0.1 M and the potential difference between the electrodes is 1.5 V. The standard electrode potential for Zinc is -0.76 V and the transfer coefficient for the electrode reaction is 0.5.

asked Jan 22 in ElectroChemistry by AlvaroZyl417 (470 points)

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1 answer 61 views

A 50 mL solution of 0.1 M Cu(NO3)2 was electrolyzed for 20 minutes. During this time, a current of 0.5 A was passed through the solution. What is the final concentration of Cu2+ ions in the solution after the electrolysis?

asked Jan 22 in ElectroChemistry by BebeU6023107 (670 points)

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1 answer 40 views

A brass alloy electrode with an area of 5 cm² is immersed in a 0.5 M NaCl solution at 25°C. Given that the standard potential of the electrode is -0.35 V versus a standard hydrogen electrode, calculate the corrosion current density of the electrode in the given environment using Tafel extrapolation.

asked Jan 22 in ElectroChemistry by ChiBouton155 (610 points)

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1 answer 39 views

A battery consists of a Zinc electrode and a Copper electrode. Calculate the exchange current density at the Zinc electrode if the concentration of Zinc ion in its solution is 0.1 M and the potential difference between the electrodes is 1.5 V. The standard electrode potential for Zinc is -0.76 V and the transfer coefficient for the electrode reaction is 0.5.

asked Jan 22 in ElectroChemistry by BlytheWedgwo (570 points)

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