Electrochemical Cells
Chemistry ⇒ Redox Reactions and Electrochemistry
Electrochemical Cells starts at 11 and continues till grade 12.
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See sample questions for grade 12
A cell is constructed with the following half-cells: Fe2+/Fe (E° = -0.44 V) and Ag+/Ag (E° = +0.80 V). Which metal will be deposited at the cathode?
Calculate the cell potential at 25°C for the cell: Zn(s) | Zn2+(1.0 M) || Cu2+(0.01 M) | Cu(s). E°cell = 1.10 V. (Use the Nernst equation: Ecell = E°cell - (0.059/2) log([Cu2+]/[Zn2+]))
Calculate the standard cell potential for a cell with the following half-reactions: Zn2+ + 2e- → Zn(s) E° = -0.76 V; Cu2+ + 2e- → Cu(s) E° = +0.34 V.
Calculate ΔG° for a cell reaction where n = 2, E°cell = 1.10 V, and F = 96500 C/mol.
Describe the construction and working of a Daniell cell.
Describe the function of the salt bridge in a galvanic cell.
Describe the role of inert electrodes in electrochemical cells.
Explain why platinum is often used as an electrode in electrochemical cells involving gases or ions only.
Explain why the cell potential decreases as the cell operates.
Explain why the salt bridge is necessary in an electrochemical cell.
State the direction of electron flow in a galvanic cell.
State the main difference between a galvanic cell and an electrolytic cell.
State the relationship between Gibbs free energy change (ΔG) and cell potential (Ecell).
Write the cell notation for a galvanic cell consisting of a zinc electrode in ZnSO4 solution and a copper electrode in CuSO4 solution.
