Recent questions in ElectroChemistry

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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 Feb 3 in ElectroChemistry by CletaF793120 (2.8k points)

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1 answer 58 views

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 Feb 3 in ElectroChemistry by MerissaGxv8 (1.7k points)

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1 answer 44 views

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 Feb 3 in ElectroChemistry by LannyNewell (1.8k points)

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1 answer 65 views

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 Feb 3 in ElectroChemistry by CooperPallad (1.7k points)

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1 answer 82 views

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 Feb 3 in ElectroChemistry by DoloresLocke (1.7k points)

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1 answer 75 views

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 Feb 3 in ElectroChemistry by TrevorE07525 (2.2k points)

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1 answer 72 views

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 Feb 3 in ElectroChemistry by Linnea35385 (2.0k points)

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1 answer 81 views

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

asked Feb 3 in ElectroChemistry by XLNDorris808 (1.7k points)

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1 answer 72 views

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

asked Feb 3 in ElectroChemistry by MurrayDrew60 (1.7k points)

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1 answer 96 views

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

asked Jan 31 in ElectroChemistry by JaysonPlott5 (1.6k points)

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1 answer 87 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 Jan 30 in ElectroChemistry by PercyBanning (1.6k points)

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1 answer 83 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 MarquisMonte (1.9k points)

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1 answer 63 views

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 BarrettGriff (2.0k points)

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1 answer 64 views

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 JordanChun58 (2.3k points)

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1 answer 78 views

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 MorrisMcGahe (1.7k points)

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1 answer 66 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 RandolphNola (1.8k points)

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1 answer 66 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 JulianKnetes (2.0k points)

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1 answer 96 views

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 BuckY7205505 (1.7k points)

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1 answer 64 views

Calculate the Faraday constant for a half-cell reaction in which the electrode potential is 0.32 V and one mole of electrons are exchanged during the reaction. Express your answer in units of coulombs per mole.

asked Jan 23 in ElectroChemistry by Phillipp57B1 (2.3k points)

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1 answer 64 views

Calculate the extent of polarization for a cell in which a copper electrode is coupled with a silver electrode at 25°C. The copper electrode has a potential of -0.34 V and the silver electrode has a potential of 0.80 V. The initial concentration of copper ions and silver ions in the solution are 0.001 M and 0.01 M, respectively. The total resistance of the cell (including both the electrolyte and the external circuit) is 10 ohms. Assume that the transfer coefficient for both the copper and silver ions is 0.5, and the Faraday constant is 96,485 C/mol.

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

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