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 11
A cell is constructed with the following half-cells: Fe2+/Fe (E° = -0.44 V) and Pb2+/Pb (E° = -0.13 V). Which metal will act as the anode?
Calculate the cell potential at 25°C for a cell with the following reaction: Zn(s) + Cu2+(aq) → Zn2+(aq) + Cu(s), if [Zn2+] = 0.10 M, [Cu2+] = 1.0 M, Ecell° = 1.10 V. (Use the Nernst equation: E = E° - (0.0592/n) log Q, n = 2)
Calculate the number of moles of electrons transferred in the following reaction: 2Ag+(aq) + Cu(s) → 2Ag(s) + Cu2+(aq)
Calculate the standard cell potential (Ecell°) for a cell made of Mg(s) | Mg2+(aq) || Ag+(aq) | Ag(s), given EMg2+/Mg° = -2.37 V and EAg+/Ag° = +0.80 V.
Describe the difference between a galvanic cell and an electrolytic cell.
Describe the role of the external circuit in an electrochemical cell.
Describe what happens to the mass of the anode and cathode as a galvanic cell operates.
Explain why a salt bridge is necessary in a galvanic cell but not in a single half-cell.
Explain why the cell potential decreases as a galvanic cell operates over time.
Given the cell: Ag(s) | Ag+(aq) || Cu2+(aq) | Cu(s), if EAg+/Ag° = +0.80 V and ECu2+/Cu° = +0.34 V, which metal is oxidized?
Given the following cell: Zn(s) | Zn2+(aq) || Cu2+(aq) | Cu(s), which half-cell undergoes reduction?
In a cell notation, which electrode is written on the left side?
In a cell, if the anode is made of magnesium and the cathode is made of silver, which metal will lose mass during operation?
State one reason why platinum is often used as an electrode in electrochemical cells.
State the function of the salt bridge in a galvanic cell.
State the relationship between Gibbs free energy change (ΔG) and cell potential (Ecell).
What is the main purpose of a salt bridge in an electrochemical cell?
