Electrochemical Cells
Physics ⇒ Electricity and Magnetism
Electrochemical Cells starts at 10 and continues till grade 12.
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See sample questions for grade 12
A cell is constructed with the following half-cells: Ag⁺/Ag (E° = +0.80 V) and Fe²⁺/Fe (E° = -0.44 V). Calculate the standard cell potential.
A cell is constructed with the following half-cells: Pb²⁺/Pb (E° = -0.13 V) and Ni²⁺/Ni (E° = -0.25 V). Which metal will be oxidized?
Calculate the number of moles of electrons transferred when 1 mole of Zn is oxidized to Zn²⁺.
Calculate the standard cell potential (E°cell) for a cell made of Zn/Zn²⁺ (E° = -0.76 V) and Cu/Cu²⁺ (E° = +0.34 V).
Describe the main difference between a galvanic cell and an electrolytic cell.
Explain why a salt bridge is necessary in a galvanic cell.
Explain why the anode is negative in a galvanic cell but positive in an electrolytic cell.
If the concentration of Zn²⁺ ions in a Daniell cell is increased, what happens to the cell potential?
In a Daniell cell, zinc is used as the anode and copper as the cathode. Which metal is oxidized?
State the effect of increasing temperature on the cell potential of a galvanic cell, assuming the reaction is exothermic.
State the relationship between Gibbs free energy change (ΔG) and cell potential (Ecell) for an electrochemical cell.
The overall cell reaction in a Daniell cell is Zn(s) + Cu²⁺(aq) → Zn²⁺(aq) + Cu(s). Which species is reduced?
Write the Nernst equation for a general electrochemical cell reaction.
