Quiz  /  Fuel Cell Class 11 MCQ Questions With Answers

  • 1. 
    What is an electrolyte?

  • An electric current
  • The splitting of ionic compounds
  • A solution containing ions which allows current to flow.
  • The salts in drinking water.

  • 2. 
    What is a battery?

  • A single cell
  • Two or more cells connected in series
  • AA or AAA
  • An alkaline substance

  • 3. 
    What are the products in a hydrogen fuel cell?

  • Water
  • Oxygen
  • Hydrogen

  • 4. 
    What is the main reason why hydrogen is more difficult to store than diesel?

  • Hydrogen is a gas at room temperature but diesel is a liquid
  • Hydrogen can be liquefied by cooling it
  • Hydrogen can be stored under pressure

  • 5. 
    State three disadvantages of hydrogen fuel cells

  • Do not need to be recharged, no pollutants are produced, can be different sizes for different uses
  • Hydrogen is highly flammable, hydrogen is sometimes produced through non-renewable means, hydrogen is difficult to store

  • 6. 
    What does the potential difference of a cell depend on?

  • The anode and cathode.
  • The type of electrolyte and fuel
  • Whether it's alkali or not
  • The type of electrode and the electrolyte.

  • 7. 
    What happens to hydrogen molecules in a hydrogen-oxygen fuel cell?

  • They form hydrogen ions, H+ , and electrons, e-
  • They form hydrogen ions, H+ , and electrons, e+
  • They form hydrogen atoms, H

  • 8. 
    What is produced by a hydrogen-oxygen fuel cell?

  • Water and Carbon Dioxide
  • Carbon Dioxide
  • Water

  • 9. 
    State three advantages of hydrogen fuel cells

  • Do not need to be recharged, no pollutants are produced, can be different sizes for different uses
  • Hydrogen is highly flammable, hydrogen is sometimes produced through non-renewable means, hydrogen is difficult to store

  • 10. 
    What is the fuel for a fuel cell?

  • Oxygen
  • Hydrogen-rich Fuels
  • Ozone
  • Water

  • 11. 
    How does the reactivity of the metal electrodes affect the size of the potential difference?

  • The lower the difference in reactivity, the greater the potential difference.
  • The greater the difference in reactivity, the lower the potential difference.
  • The greater the difference in reactivity, the greater the potential difference.
  • The lower the difference in reactivity, the lower the potential difference.

  • 12. 
    Complete the equation which occurs at the positive electrode of a hydrogen fuel cell O₂ + 2H₂O →

  • OH⁻
  • 2OH⁻
  • 3OH⁻
  • 4OH⁻

  • 13. 
    Why can some cells not be recharged?

  • Because the reaction is not reversible
  • Because the reaction is reversible
  • Because the reactant is used up
  • Because the products are used up

  • 14. 
    What happens to oxygen molecules in a hydrogen-oxygen fuel cell?

  • They react with electrons to form oxide ions, O2-
  • They react with hydrogen ions to form hydroxide ions, OH-
  • They react with hydrogen ions and electrons to form water

  • 15. 
    Fuel cells produce

  • Fossil Fuels
  • Hydrogen gas
  • Electricity
  • Gasoline

  • 16. 
    In non-rechargeable cells, why do the chemical reactions stop over time?

  • One of the reactants becomes used up.
  • The energy has depleted.
  • The products are oxidised.
  • The electrodes become reactive.

  • 17. 
    Which of these is a disadvantage of cars driven by hydrogen-oxygen fuel cells rather than by petrol engines?

  • They have fewer moving parts
  • There are fewer suitable filling stations
  • They emit little pollution

  • 18. 
    What type of reaction takes place in a chemical cell

  • Exothermic
  • Endothermic
  • No reaction occurs

  • 19. 
    In a hydrogen fuel cell used to power a car, where does the oxygen come from?

  • The air
  • A catalyst
  • The fuel

  • 20. 
    Complete the equation which occurs at the negative electrode of a hydrogen fuel cell 2H₂ + 4OH⁻ →

  • H₂O + 4e⁻
  • 4H₂O + e⁻
  • 4H₂O + 4e⁻
  • 3H₂O + 2e⁻

  • 21. 
    What are the main components of a chemical cell?

  • An anode, a cathode
  • An anode, a cathode and an electrolyte
  • An anode and an electrolyte
  • A cathode and an electrolyte

  • 22. 
    Why does the voltage from a chemical cell that is connected in a circuit with a lamp eventually reach zero?

  • The lamp breaks
  • One of the reactants is used up
  • The circuit becomes broken

  • 23. 
    What is a strength of using hydrogen-oxygen fuel cells in manned spacecraft, compared to using chemical cells?

  • They produce electricity
  • They produce water that the astronauts can drink
  • They produce a voltage

  • 24. 
    The half-equation for the reaction occurring at the (+) electrode in a hydrogen-oxygen fuel which has an alkaline electrolyte would be

  • H2(g) + 2OH-(aq)→ 2H2O(l) + 2e-
  • H2(g) → 2H+(g) + 2e-
  • O2(g) + 4H+(aq) + 4e- → 2H2O(l)
  • O2(g) + 2H2O(l) + 4e- → 4OH- (aq)

  • 25. 
    A fuel cell can be constructed that uses the two half-reactions as shown.Which one of the following would occur at the negative electrode of the cell as it generates electricity?

  • production of H+
  • formation of H2O
  • consumption of CO2
  • reduction of CH3OH

  • 26. 
    In a fuel cell based on the oxidation of methane, the equation for the anode half-reaction is:CH4(g) + 2H2O(l) → CO2(g) + 8H+(aq) + 8e-The corresponding equation for the half-reaction at the cathode is

  • 2H2O(l) + 4e- → 4H+(aq) + O2(g)
  • 4H+(aq) + O2(g) → 2H2O(l)
  • 2H2O(l) → 4H+(aq) + O2 (g) + 4e-
  • 4H+(aq) + O2(g) + 4e- → 2H2O(l)

  • 27. 
    A simplified diagram of the phosphoric acid fuel cell (PAFC), and their half-reactions are shown. The cell operates at 190oC using an electrolyte of liquid phosphoric acid.During operation of the PAFC, electrode I is

  • positively charged, and the pH near the electrode will increase
  • positively charged, and the pH near the electrode will decrease
  • negatively charged, and the pH near the electrode will increase
  • negatively charged, and the pH near the electrode will decrease

  • 28. 
    The energy released in a chemical reaction is directly converted to electrical energy in al

  • solar cell
  • electrolytic cell
  • fossil-fuel power station
  • hydrogen/oxygen fuel cell

  • 29. 
    A fuel cell currently under development for powering small electronic devices is based on the reaction of methanol and oxygen using an acidic electrolyte. The reductant in the cell reaction and the half-reaction at the anode are

  • Methanol; O2(g) + 4H+(aq) + 4e- → 2H2O(l)
  • Oxygen; O2(g) + 4H+(aq) + 4e- → 2H2O(l)
  • Methanol; CH3OH(g) + H2O(l) → CO2(g) + 6H+(aq) + 6e-
  • Oxygen; CH3OH(g) + H2O(l) → CO2(g) + 6H+(aq) + 6e-

  • 30. 
    Which one of the following state is true for both fuel cells and rechargeable cells?

  • All reactants are stored within the cell.
  • Reaction products are continuously removed from the cell.
  • Electrons pass from the reductant to the anode as electricity is produced.
  • Electrical energy is converted to chemical energy as the cell is recharged.
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