Batteries and Fuel Cells
Chemistry ⇒ Redox Reactions and Electrochemistry
Batteries and Fuel Cells starts at 12 and continues till grade 12.
QuestionsToday has an evolving set of questions to continuously challenge students so that their knowledge grows in Batteries and Fuel 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 12
A certain battery has a cell potential of 2.0 V. If the battery delivers a current of 1.5 A for 2 hours, calculate the total charge delivered.
A Daniell cell is constructed using Zn and Cu electrodes. If the concentration of Zn2+ is increased, what happens to the cell potential?
A fuel cell has an efficiency of 60%. If the enthalpy change for the reaction is −285 kJ/mol, calculate the maximum electrical work obtainable per mole of fuel.
A fuel cell is operating with hydrogen and oxygen gases at 25°C. If the partial pressure of H2 is increased, what is the effect on the cell voltage?
Calculate the cell potential for a cell constructed with the following half-cells at 25°C: Ag+(aq) + e− → Ag(s), E° = +0.80 V; Cu2+(aq) + 2e− → Cu(s), E° = +0.34 V. (Assume standard conditions.)
Describe one advantage and one disadvantage of lithium-ion batteries.
Describe the main difference between a battery and a fuel cell.
Describe the role of the separator in a battery.
Explain the term 'memory effect' in the context of batteries.
Explain why fuel cells are considered more efficient than conventional combustion engines.
Explain why primary cells cannot be recharged.
Explain why the voltage of a battery decreases as it discharges.
In a lead-acid battery, the overall cell reaction during discharge is: Pb(s) + PbO2(s) + 2H2SO4(aq) → 2PbSO4(s) + 2H2O(l). Which substance is reduced?
State one environmental advantage of using hydrogen-oxygen fuel cells over conventional fossil fuel combustion.
State one reason why batteries may lose capacity over time even if they are rechargeable.
State the main reason why mercury cells provide a constant voltage during their lifetime.
The standard cell potential (E°cell) of a Daniell cell is 1.10 V. If the cell is represented as Zn(s) | Zn2+(aq) || Cu2+(aq) | Cu(s), which electrode acts as the anode?
A certain battery is constructed using the following half-cells at 25°C:
Half-cell 1: Fe2+(aq) + 2e− → Fe(s), E° = −0.44 V
Half-cell 2: Ag+(aq) + e− → Ag(s), E° = +0.80 V
Calculate the standard cell potential (E°cell) for this battery and identify which metal acts as the anode.
A lithium-ion battery has a standard cell potential (E°cell) of 3.7 V. If the battery is fully charged and can deliver a total of 10,000 C of charge, calculate the maximum amount of electrical energy (in kJ) that can be obtained from the battery.
A nickel-metal hydride (NiMH) battery is being considered for use in a hybrid vehicle. Discuss two advantages and one disadvantage of using NiMH batteries in this application.
