Galvanic Cells

Chemistry ⇒ Redox Reactions and Electrochemistry

Galvanic Cells starts at 11 and continues till grade 12. QuestionsToday has an evolving set of questions to continuously challenge students so that their knowledge grows in Galvanic Cells. How you perform is determined by your score and the time you take. When you play a quiz, your answers are evaluated in concept instead of actual words and definitions used.

See sample questions for grade 11

A Galvanic cell is constructed using Fe and Ag electrodes. Given E°(Fe²⁺/Fe) = -0.44 V and E°(Ag⁺/Ag) = +0.80 V, which electrode is the cathode?

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 deposited at the cathode?

A Galvanic cell is constructed with the following half-cells: Pb²⁺(aq) + 2e⁻ → Pb(s) E° = -0.13 V; Ag⁺(aq) + e⁻ → Ag(s) E° = +0.80 V. Calculate the standard cell potential.

A student sets up a Galvanic cell with the following cell notation: Fe(s) | Fe²⁺(aq) || Cu²⁺(aq) | Cu(s). Which metal will be oxidized?

Calculate the number of electrons transferred in the overall reaction for a Galvanic cell with the following half-reactions: Zn(s) → Zn²⁺(aq) + 2e⁻ and Cu²⁺(aq) + 2e⁻ → Cu(s).

Calculate the standard cell potential for a Galvanic cell with the following half-reactions: Mg²⁺ + 2e⁻ → Mg(s) E° = -2.37 V; Cu²⁺ + 2e⁻ → Cu(s) E° = +0.34 V.

Describe the role of the salt bridge in preventing polarization in a Galvanic cell.

Describe what happens to the ions in the salt bridge during the operation of a Galvanic cell.

Describe what happens to the mass of the anode and cathode during the operation of a Galvanic cell.

Explain why a salt bridge is necessary in a Galvanic cell.

Explain why the anode in a Galvanic cell is negative.

Explain why the cell potential becomes zero when a Galvanic cell reaches equilibrium.

If the standard reduction potentials are E°(Zn²⁺/Zn) = -0.76 V and E°(Cu²⁺/Cu) = +0.34 V, what is the standard cell potential for the Zn-Cu Galvanic cell?

In a standard Zn-Cu Galvanic cell, which metal acts as the anode?

Name the device used to connect the two half-cells in a Galvanic cell and maintain electrical neutrality.

State the cell reaction for a Galvanic cell made of Zn and Cu electrodes in their respective 1 M solutions.

State the effect on the cell potential if the concentration of the ion in the cathode half-cell is increased.

What is the purpose of the external wire in a Galvanic cell?

A Galvanic cell is constructed using the following half-cells: MnO₄^-(aq) + 8H⁺(aq) + 5e^- → Mn²⁺(aq) + 4H₂O(l) E° = +1.51 V and Fe²⁺(aq) → Fe³⁺(aq) + e^- E° = +0.77 V. Write the balanced overall cell reaction and calculate the standard cell potential.

A Galvanic cell is constructed with the following cell notation: Ni(s) | Ni²⁺(aq, 1.0 M) || Pb²⁺(aq, 1.0 M) | Pb(s). Given E°(Ni²⁺/Ni) = -0.23 V and E°(Pb²⁺/Pb) = -0.13 V, which electrode will increase in mass as the cell operates?