Questions on Electrolytic Cells
Electrolytic Cells – Multiple Choice Questions
Questions
1. What is the primary function of an electrolytic cell?
A) To produce electrical energy from a chemical reaction
B) To measure voltage between two electrodes
C) To drive a nonspontaneous chemical reaction using electrical energy
D) To calculate the Gibbs free energy
E) To store thermal energy
-- Ads --
2. Which of the following is required for an electrolytic cell to operate?
A) Salt bridge
B) External power source
C) Spontaneous reaction
D) Photons
E) Fuel
3. In an electrolytic cell, the anode is:
A) Positive and the site of reduction
B) Negative and the site of oxidation
C) Positive and the site of oxidation
D) Neutral
E) The electrode that produces electrons
4. What happens at the cathode in an electrolytic cell?
A) Oxidation
B) Electrons are lost
C) Reduction
D) Hydrogen gas is always released
E) Electrons are emitted into solution
5. What is the role of the power supply in an electrolytic cell?
A) To provide resistance
B) To remove electrons from the cell
C) To supply the energy needed to drive the reaction
D) To neutralize the products
E) To balance charges
6. Which of the following is an example of electrolysis?
A) Combustion of methane
B) Decomposition of water into H₂ and O₂
C) Boiling water
D) Melting of ice
E) Neutralization of an acid
7. In electrolysis of molten NaCl, which product forms at the cathode?
A) Na⁺
B) Cl⁻
C) Na
D) Cl₂
E) H₂
8. Which product forms at the anode during electrolysis of molten NaCl?
A) Cl₂ gas
B) Na metal
C) Na⁺
D) H₂ gas
E) O₂ gas
9. What is typically used as the electrolyte in an electrolytic cell?
A) Water
B) Inert metal
C) Ionic compound in molten or aqueous form
D) Plastic
E) Nonpolar solvent
10. Which electrode is connected to the negative terminal of the power supply in an electrolytic cell?
A) Cathode
B) Anode
C) Salt bridge
D) Electrolyte
E) Voltmeter
11. The electrolysis of water produces which gases?
A) Hydrogen and nitrogen
B) Oxygen and hydrogen
C) Hydrogen and carbon dioxide
D) Oxygen and methane
E) Chlorine and oxygen
12. The quantity of substance produced in electrolysis is proportional to:
A) Voltage squared
B) Resistance
C) Current and time
D) Mass of electrodes
E) Pressure
13. Faraday’s First Law of Electrolysis states:
A) Charge is inversely proportional to time
B) Electrons flow from cathode to anode
C) The mass of a substance is proportional to the quantity of electric charge
D) Electrolysis only occurs in aqueous solutions
E) Anode is always negative
14. In electroplating, the object to be plated is placed at the:
A) Anode
B) Cathode
C) Power supply
D) Electrolyte
E) Middle of the cell
15. What is the unit of electric charge used in electrolysis calculations?
A) Joule
B) Volt
C) Coulomb
D) Ohm
E) Ampere
16. Which of the following can be electroplated?
A) Gas
B) Wood
C) Plastic without treatment
D) Metal objects
E) Paper
17. Electrolysis of aqueous solutions may produce different products compared to molten compounds due to:
A) The use of solid electrodes
B) The presence of water
C) Lack of temperature control
D) Lower voltage
E) High resistance
18. Which species is more likely to be reduced during aqueous electrolysis of NaCl?
A) Na⁺
B) Cl⁻
C) H₂O
D) NaCl
E) O₂
19. What is the function of inert electrodes like platinum in electrolytic cells?
A) Participate in the redox reaction
B) Provide voltage
C) Provide a surface for redox reactions without being consumed
D) Prevent ion movement
E) Create electric current
20. How many Faradays are required to deposit 1 mol of aluminum (Al³⁺)?
A) 1
B) 2
C) 3
D) 6
E) 0.5
Answers and Explanations
1. C – Electrolytic cells use electrical energy to drive nonspontaneous reactions.
2. B – An external power source is essential.
3. C – In electrolytic cells, the anode is positive and oxidation occurs.
4. C – Reduction always occurs at the cathode.
5. C – The power source supplies energy to move electrons.
6. B – Water decomposition by electricity is electrolysis.
7. C – Na⁺ gains electrons to form Na metal at the cathode.
8. A – Cl⁻ loses electrons to form Cl₂ gas at the anode.
9. C – Electrolytes are ionic compounds in molten/aqueous form.
10. A – The cathode connects to the negative terminal in electrolytic cells.
11. B – Electrolysis of water yields H₂ and O₂.
12. C – Amount of product ∝ current × time.
13. C – Faraday’s law links mass and electric charge.
14. B – In electroplating, the object to be plated is the cathode.
15. C – Coulomb (C) is the unit of electric charge.
16. D – Metal objects can be electroplated.
17. B – Water competes with ions for reduction/oxidation.
18. C – Water is easier to reduce than Na⁺ in aqueous solution.
19. C – Inert electrodes act as surfaces without reacting.
20. C – Al³⁺ + 3e⁻ → Al; needs 3 Faradays per mole.
Dive into the groundbreaking science of neurotransmitters—your brain’s invisible architects—in Chemical Harmony: How Neurotransmitters Shape Our Lives (2025). This meticulously researched book reveals how serotonin, dopamine, GABA, and other brain chemicals silently orchestrate every aspect of your existence, from decision-making and relationships to mental health and emotional resilience.Click here to buy
Share Online!
