The standard potential for the following galvanic cell is +0.90 V: 3 Cu²⁺(aq) + 2 Ga(s) → 3 Cu(s) + 2 Ga³⁺(aq). Given that the standard reduction potential for the Cu²⁺/Cu half-cell is +0.34 V, what is the standard reduction potential for the Ga³⁺/Ga half-cell?

Consider the following substances: Fe(s), PbO2(s), H+(aq), Al(s), Ag(s), Cr2O72-(aq).(d) Which substances can be oxidized by Cu2+(aq)? Which can be reduced by H2O2(aq)?

Which of the following represents the balanced equation for the overall redox reaction between Fe³⁺(aq) and Cr(s) based on their standard reduction potentials?

Use the standard half-cell potentials listed below to calculate the standard cell potential for the following reaction occurring in an electrochemical cell at 25°C. (The equation is balanced.)Pb(s) + Br2(l) → Pb2+(aq) + 2 Br-(aq)Given the standard reduction potentials:Pb2+(aq) + 2 e- → Pb(s) E° = -0.13 VBr2(l) + 2 e- → 2 Br-(aq) E° = +1.07 VWhat is the standard cell potential (E°cell) for the reaction?

Use the table of standard reduction potentials to calculate the equilibrium constant at standard temperature (25 °C) for the reaction: Fe(s) + Ni²⁺(aq) → Fe²⁺(aq) + Ni(s). Which of the following is the correct equilibrium constant (K)?

Using standard reduction potentials, calculate the standard emf for the following reaction: Co(s) + 2Co³⁺(aq) → 3Co²⁺(aq). What is the standard emf of this reaction?

What is the value (in V) of E°cell for the reaction Cu²⁺ (aq) + Fe (s) → Cu (s) + Fe²⁺ (aq) given the standard reduction potentials: Cu²⁺/Cu = +0.34 V and Fe²⁺/Fe = -0.44 V?