Recent questions in ElectroChemistry

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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 2 days ago in ElectroChemistry by GabriellaJai (250 points)

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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 2 days ago in ElectroChemistry by NestorSeccom (410 points)

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Calculate the overpotential of a lead electrode in contact with a solution containing [Pb2+] = 0.001 M when the temperature is 298 K. Given that the standard potential of the Pb2+ / Pb electrode is -0.13 V and the exchange current density is 0.015 A/m2.

asked 2 days ago in ElectroChemistry by JoeyGkg21308 (350 points)

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Calculate the overpotential for the reduction reaction of Ag+ to Ag on a silver electrode at 25°C with a current density of 0.5 A/cm2. The standard reduction potential of Ag+ to Ag is 0.799 V vs. the standard hydrogen electrode. The activation energy for this reaction is 65.0 kJ/mol, the transfer coefficient is 0.4 and the reaction order is 1.5.

asked 2 days ago in ElectroChemistry by AllisonMcRob (670 points)

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Calculate the overpotential (in millivolts) for the reduction of Cu2+ to Cu on a copper electrode at 25°C, given that the standard reduction potential of Cu2+ to Cu is +0.34 V and the actual voltage is 0.32 V.

asked 2 days ago in ElectroChemistry by DorethaBeam6 (710 points)

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Calculate the number of electrons transferred when a solution containing 0.25 M Ni(NO3)2 is electrolyzed using a current of 0.50 A for 2.0 hours. The reaction taking place is Ni2+ (aq) + 2e- --> Ni (s).

asked 2 days ago in ElectroChemistry by GarfieldLoui (530 points)

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Calculate the number of electrons transferred when 1 mole of magnesium is oxidized to form magnesium ions in an electrochemical cell. The balanced half-reaction is Mg → Mg2+ + 2e-.

asked 2 days ago in ElectroChemistry by KristyDobos (430 points)

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Calculate the number of electrons transferred in the following reaction: Cu(s) + 2AgNO3(aq) → Cu(NO3)2(aq) + 2Ag(s) Hint: In order to balance the equation, you'll need to add electrons to one side of the reaction.

asked 2 days ago in ElectroChemistry by IrisHammond9 (470 points)

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Calculate the number of electrons transferred in the electrochemical reaction when a solution of silver nitrate is added to a copper electrode and a salt bridge is used to complete the circuit.

asked 2 days ago in ElectroChemistry by BradfordKins (330 points)

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Calculate the number of electrons transferred during the following redox reaction: Cu(s) + 2Ag+ --> Cu2+ + 2Ag(s)

asked 2 days ago in ElectroChemistry by MohammedBris (530 points)

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Calculate the number of electrons transferred during the following electrochemical reaction: Mg(s) + 2H+(aq) → Mg2+(aq) + H2(g)

asked 2 days ago in ElectroChemistry by MichaleChen (470 points)

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What is the oxidation state of nitrogen in ammonium nitrate (NH4NO3)?

asked 5 days ago in ElectroChemistry by CliffHalvors (350 points)

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1 answer 45 views

Calculate the number of electrons transferred when a solution containing 0.50 mol of HCl reacts with 0.50 mol of NaOH in a redox reaction.

asked 5 days ago in ElectroChemistry by Lucas40K2221 (530 points)

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1 answer 54 views

Calculate the mass of silver (Ag) that will be deposited on the cathode during electrolysis if a current of 2.5 A is passed through a solution of silver nitrate (AgNO3) for 3 hours.

asked Jan 23 in ElectroChemistry by Jeannie04C30 (530 points)

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Calculate the Gibbs free energy change for the following electrochemical reaction at 298 K:Mg(s) + 2H+(aq) → Mg2+(aq) + H2(g)Given:Standard Gibbs free energy change of formation of Mg2+: -466 kJ/molStandard Gibbs free energy change of formation of H+: 0 kJ/molStandard Gibbs free energy change of formation of H2: 0 kJ/molStandard Gibbs free energy change of formation of Mg: 0 kJ/mol

asked Jan 23 in ElectroChemistry by BobRiv48789 (370 points)

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Calculate the Gibbs free energy change for the following electrochemical reaction at 298 K:2Fe³⁺(aq) + 2e⁻ → 2Fe²⁺(aq)Given that the standard Gibbs energy of formation of Fe³⁺(aq) is -290.5 kJ/mol and that of Fe²⁺(aq) is -91.2 kJ/mol.

asked Jan 23 in ElectroChemistry by JorgDesir647 (660 points)

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Calculate the Gibbs free energy change for the electrochemical reaction: Zn(s) + Cu2+(aq) → Zn2+(aq) + Cu(s) Given the standard reduction potentials: E°(Cu2+/Cu) = 0.34 V E°(Zn2+/Zn) = -0.76 V Assuming standard conditions of 1 M concentration and 1 atm pressure at 25°C.

asked Jan 23 in ElectroChemistry by AbrahamMaruf (550 points)

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1 answer 37 views

Calculate the Gibbs free energy change for the electrochemical reaction where zinc metal (Zn) is oxidized by aqueous hydrogen ions (H+) to form aqueous zinc ions (Zn2+) and hydrogen gas (H2) at 298 K, given that the standard reduction potential of Zn2+/Zn is -0.76 V and the standard hydrogen electrode potential is 0 V.

asked Jan 23 in ElectroChemistry by ZVSLourdes7 (590 points)

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1 answer 46 views

Calculate the Gibbs free energy change for the electrochemical reaction where Fe(s) is oxidized to Fe3+(aq) and Br2(l) is reduced to Br-(aq) with the help of the following half-reactions: Fe3+(aq) + e- ⇌ Fe2+(aq) E° = 0.771 VBr2(l) + 2e- ⇌ 2Br-(aq) E° = 1.087 V

asked Jan 23 in ElectroChemistry by BennieFll738 (410 points)

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Calculate the Gibbs free energy change for the electrochemical reaction in which 2 moles of electrons are transferred from a zinc electrode to a copper electrode. The standard reduction potentials are E°(Cu²⁺/Cu) = 0.34 V and E°(Zn²⁺/Zn) = -0.76 V. What is the spontaneity of the reaction under standard conditions?

asked Jan 23 in ElectroChemistry by EloyHakala8 (330 points)

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