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Calculate the standard electrode potential of the half-cell reaction Ag+ + e- → Ag, given that the standard reduction potential of Ag+ is 0.80 V.

asked Feb 3 in ElectroChemistry by KristeenN708 (2.1k points)

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Calculate the standard electrode potential of the following reaction: Cu2+(aq) + 2e- ⇌ Cu(s) Given that the standard reduction potential of Cu2+(aq) is +0.34 V and the standard electrode potential of hydrogen electrode is 0.00 V.

asked Feb 3 in Chemical thermodynamics by Lizzie32E683 (1.8k points)

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Calculate the standard electrode potential of the following cell: Zn(s) | Zn2+(aq) || Cu2+(aq) | Cu(s) Given: Eº(Zn2+(aq)/Zn(s)) = -0.76 V and Eº(Cu2+(aq)/Cu(s)) = +0.34 V.

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

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Calculate the standard electrode potential of the following cell reaction at 25°C: Cu(s) | Cu2+ (0.01 M) || Zn2+ (1.0 M) | Zn(s)

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

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Calculate the standard electrode potential of the electrode in the given electrochemical cell: Fe3+(aq) + 3e- → Fe(s) E°= -0.04V Ag+(aq) + e- → Ag(s) E°= 0.80V

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

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Calculate the standard electrode potential of the copper electrode if the standard electrode potential of the zinc electrode is -0.76 V and the standard cell potential is 1.10 V for the cell reaction: Zn(s) + Cu2+(aq) → Zn2+(aq) + Cu(s). Use the equation Eºcell=Eº cathode - Eº anode where Eºcell is the standard cell potential, Eºcathode is the standard potential for the reduction half-reaction, and Eºanode is the standard potential for the oxidation half-reaction.

asked Feb 3 in ElectroChemistry by Jeramy48117 (1.9k points)

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Calculate the standard electrode potential of copper electrode if the Cu2+ ion concentration is 1.0 M and the electrode is at 25°C. The half-cell reaction is Cu2+(aq) + 2e- → Cu(s).

asked Feb 3 in ElectroChemistry by AnibalX1615 (2.1k points)

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Calculate the standard electrode potential of an electrode that is in contact with a solution containing 0.1 M copper (II) ions and its concentration of Cu2+ ions is in equilibrium with a hydrogen electrode at 1 atm hydrogen pressure and pH = 0.

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

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1 answer 93 views

Calculate the standard electrode potential of a silver electrode (Ag) in contact with a solution containing 1.0 M AgNO3 and a hydrogen electrode (Pt) in contact with a solution containing 1.0 M HCl, given that the reduction potential of Ag+/Ag is +0.80V and the reduction potential of H+/H2 is 0.00V at 298K.

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

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Calculate the standard electrode potential of a half-cell containing F2(g) and F- ion at 25°C. The reduction potential for F2(g) is 2.87 V and the standard reduction potential for F- ion is -2.87 V.

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

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Calculate the standard electrode potential for the redox reaction: Al(s) + Fe2+(aq) → Fe(s) + Al3+(aq) at 298K, given that the standard reduction potential for Fe2+/Fe is -0.44V and Al3+/Al is -1.66V.

asked Feb 3 in Chemical thermodynamics by MargueriteSa (2.1k points)

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Calculate the standard electrode potential for the redox reaction: Zn(s) + Cu2+(aq) → Zn2+(aq) + Cu(s)if the standard electrode potentials for Zn2+/Zn and Cu2+/Cu half-cells are -0.76V and +0.34V, respectively.

asked Feb 3 in Chemical thermodynamics by ElisaWestgar (1.8k points)

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Calculate the standard electrode potential for the redox reaction: Fe3+(aq) + e- → Fe2+(aq) given that the standard reduction potential for the Fe3+(aq)/Fe2+(aq) couple is +0.77 V.

asked Feb 3 in Chemical thermodynamics by ChristelIdr7 (1.7k points)

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Calculate the standard electrode potential for the redox reaction: Fe3+(aq) + e- → Fe2+(aq) Given that the standard electrode potential for the reduction of Fe3+(aq) to Fe2+(aq) is +0.771 V and the standard electrode potential for the reduction of H+(aq) to H2(g) is 0.000 V.

asked Feb 3 in Chemical thermodynamics by ZellaSeamon3 (1.6k points)

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Calculate the standard electrode potential for the redox reaction: Cu(s) + 2Ag+(aq) → Cu2+(aq) + 2Ag(s) Given that the standard reduction potential for Ag+ is +0.80 V and for Cu2+ is +0.34 V.

asked Feb 3 in Chemical thermodynamics by JoliePeters1 (2.3k points)

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1 answer 53 views

Calculate the standard electrode potential for the redox reaction where Ag(s) is oxidized by Cu2+(aq) to form Ag+(aq) and Cu(s) given that the standard reduction potential for Ag+(aq) + e- → Ag(s) is 0.80 V and for Cu2+(aq) + 2e- → Cu(s) is 0.34 V.

asked Feb 3 in Chemical thermodynamics by TrevorE07525 (2.2k points)

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1 answer 38 views

Calculate the standard electrode potential for the redox reaction that occurs when a silver electrode is placed in a solution containing 0.1 M Ag+ ions and a platinum electrode is placed in a solution containing 0.1 M H+ ions at standard conditions. The reduction half-reaction for Ag+ is Ag+ (aq) + e- → Ag(s), and the reduction half-reaction for H+ is H+ (aq) + e- → 1/2 H2 (g).

asked Feb 3 in Chemical thermodynamics by RogerDenning (2.4k points)

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Calculate the standard electrode potential for the redox reaction between the half cells Ag/Ag+ and Cu2+/Cu at 25°C, given that the standard electrode potentials for the half cells are +0.80 V and +0.34 V respectively.

asked Feb 3 in Chemical thermodynamics by MerissaGxv8 (1.7k points)

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Calculate the standard electrode potential for the redox reaction between silver and copper ions at 298K, given that the reduction potential for the half-reaction Ag+ + e- → Ag is +0.80 V and the reduction potential for the half-reaction Cu2+ + 2e- → Cu is +0.34 V.

asked Feb 3 in Chemical thermodynamics by AnitraSchard (2.1k points)

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Calculate the standard electrode potential for the redox reaction between copper and silver ions, given the following half-equations:Cu2+(aq) + 2e- → Cu(s) E° = +0.34 VAg+(aq) + e- → Ag(s) E° = +0.80 V

asked Feb 3 in Chemical thermodynamics by EdwinLindell (1.9k points)

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