untitled

What reaction occurs at the anode?

Ag⁺/Ag = 0.80V

Ni²⁺/Ni = -0.25V

• Ag⁺ + e^- →Ag

• Ag → Ag⁺ + e^-

• Ni²⁺ + 2e^- → Ni

• Ni → Ni²⁺ + 2e^-

In the following reaction

Sn⁺² + 2Fe⁺³ → Sn⁺⁴ + 2Fe⁺²

the oxidizing agent is....

• Sn⁺⁴

• Sn⁺²

• Fe⁺³

• Fe⁺²

Which of the species strong oxidizing agent?

Cl₂(g) + 2e → 2Cl^-(aq) E^ocell = + 1.36 V

Cu²⁺(aq) + 2e → Cu(s) E^ocell = + 0.34 V

Ni²⁺(aq) + 2e → Ni(s) E^ocell = – 0.25 V

Ca²⁺(aq) + 2e → Ca(s) E^ocell = – 2.87 V

• Cl₂(g)

• Cu²⁺(aq)

• Ni²⁺(aq)

• Ca²⁺(aq)

Calculate standard cell potential for this equation:

Zn²⁺(aq) + 2e → Zn(s) Eº = – 0.76 V

Cd²⁺(aq) + 2e → Cd(s) Eº = – 0.40 V

• E^ocell = -0.36 V

• E^ocell = -1.16 V

• E^ocell = +1.16 V

• E^ocell = +0.36 V

Reactions in galvanic/voltaic cells are

• spontaneous, redox reactions
• non-spontaneous, redox reactions
• spontaneous, non-redox reactions
• non-spontaneous, non-redox reactions

_______ is the reference electrode that can be used as an anode or a cathode depends on the half-cell to with it is coupled.

• Standard electrode potential

• Standard hydrogen electrode

• Standard cell potential

• Electrode potential

What reaction occurs at the anode?

• Ag⁺ + e^- →Ag
• Ag → Ag⁺ + e^-
• Ni²⁺ + 2e^- → Ni
• Ni → Ni²⁺ + 2e^-

In a Galvanic Cell, the salt bridge...

• completes the circuit so that electrons can flow through the wire

• maintains charge balance

• is soaked in an unreactive electrolyte such as KNO₃

• all of the above