Galvanic Cells
Chemistry ⇒ Redox Reactions and Electrochemistry
Galvanic Cells starts at 11 and continues till grade 12.
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A Galvanic cell is constructed with the following half-cells: Ag⁺(aq) + e⁻ → Ag(s), E° = +0.80 V; Cu²⁺(aq) + 2e⁻ → Cu(s), E° = +0.34 V. Which metal is oxidized?
Calculate the number of moles of electrons transferred in the following cell reaction: 2Ag⁺(aq) + Cu(s) → 2Ag(s) + Cu²⁺(aq).
Describe the role of the external circuit in a Galvanic cell.
Describe what happens to the mass of the anode and cathode during the operation of a typical Galvanic cell.
Explain why a Galvanic cell stops working after some time.
Explain why the salt bridge is necessary in a Galvanic cell.
If the standard reduction potentials are: E°(Cu²⁺/Cu) = +0.34 V and E°(Zn²⁺/Zn) = -0.76 V, what is the standard cell potential for a Zn-Cu Galvanic cell?
In a standard Zn-Cu Galvanic cell, which metal acts as the anode?
State one difference between a Galvanic cell and an electrolytic cell.
State the Nernst equation for calculating the cell potential under non-standard conditions.
The salt bridge in a Galvanic cell serves to ________.
What is the purpose of using a platinum electrode in a Galvanic cell?
Write the balanced overall cell reaction for a Galvanic cell with the following half-reactions: Zn(s) → Zn²⁺(aq) + 2e⁻ and Cu²⁺(aq) + 2e⁻ → Cu(s).
A Galvanic cell is constructed using Fe2+/Fe and Pb2+/Pb half-cells. The standard reduction potentials are: E°(Fe2+/Fe) = -0.44 V and E°(Pb2+/Pb) = -0.13 V. Calculate the standard cell potential and identify which electrode acts as the anode.
A Galvanic cell is constructed with the following half-cells: MnO4-(aq) + 8H+(aq) + 5e- → Mn2+(aq) + 4H2O(l), E° = +1.51 V; Fe3+(aq) + e- → Fe2+(aq), E° = +0.77 V. Write the balanced overall cell reaction and calculate the standard cell potential.
A student sets up a Galvanic cell with the following cell notation: Mg(s) | Mg2+(aq, 1 M) || Ag+(aq, 1 M) | Ag(s). Given E°(Mg2+/Mg) = -2.37 V and E°(Ag+/Ag) = +0.80 V, calculate the standard cell potential and write the balanced overall cell reaction.
Explain why the cell potential of a Galvanic cell decreases as the reaction proceeds toward equilibrium.
In a Galvanic cell, the standard cell potential is positive, but the cell is not producing any current. What is the most likely reason for this observation?
