Electrochemistry and Redox Reactions - Question Bank

1. The unit of electrical conductance is:
A) Ohm
B) Siemens
C) Volt
D) Ampere
2. Which of the following is an example of an electrolytic refining process?
A) Production of aluminum from bauxite
B) Purification of copper
C) Charging of a lead-acid battery
D) Operation of a dry cell
3. What is the standard cell potential (E°_cell) of a galvanic cell?
A) The potential difference under non-standard conditions
B) The potential difference at equilibrium
C) The potential difference under standard conditions (1 M concentration, 1 atm pressure, 25°C)
D) The potential difference required for electrolysis
4. Electrochemical impedance spectroscopy (EIS) is a technique used to study:
A) The rate of chemical reactions
B) The electrical properties of electrochemical interfaces
C) The thermal conductivity of electrolytes
D) The optical properties of solutions
5. What is the oxidation state of carbon in methane (CH4)?
A) +4
B) -4
C) 0
D) +1
6. The Nernst equation is derived from the relationship between Gibbs free energy change and:
A) Cell potential
B) Concentration
C) Temperature
D) Pressure
7. Which of the following is a strong electrolyte?
A) Pure water
B) Sugar solution
C) Dilute sulfuric acid
D) Ethanol
8. What happens to the anode in a typical galvanic cell made of two different metals and their salt solutions?
A) It dissolves and loses mass
B) It gains mass
C) It remains unchanged
D) It becomes coated with another metal
9. The process of depositing a thin layer of a desired metal onto another metal using electrolysis is called:
A) Electrorefining
B) Electrosynthesis
C) Electroplating
D) Electrogravimetry
10. Which of the following is a unit of electric charge?
A) Volt
B) Ampere
C) Ohm
D) Coulomb
11. What is the primary role of the Daniell cell in electrochemistry education?
A) Demonstrating electrolysis
B) Illustrating a spontaneous redox reaction generating electricity
C) Explaining Faraday's laws
D) Showing the process of electroplating
12. In a fuel cell, the reactants are supplied externally and continuously, while the products are removed. This allows for:
A) Recharging of the cell
B) Continuous operation
C) Intermittent power generation
D) Storage of energy
13. What is the oxidation state of nitrogen in HNO3?
A) +1
B) +3
C) +5
D) -3
14. Which of the following metals has the lowest standard electrode potential and is thus the strongest reducing agent?
A) Copper (Cu)
B) Zinc (Zn)
C) Lithium (Li)
D) Silver (Ag)
15. The rate of ionic migration in an electrolyte is proportional to the applied electric field strength. This is a consequence of:
A) Faraday's Law
B) Kohlrausch's Law
C) Ohm's Law for electrolytes
D) Nernst Equation
16. What is the unit of electrochemical potential difference?
A) Ampere
B) Ohm
C) Volt
D) Faraday
17. Which phenomenon is responsible for the rusting of iron?
A) Neutralization reaction
B) Electrochemical corrosion
C) Thermal decomposition
D) Photochemical reaction
18. What is the overall reaction in a lead-acid battery during discharge?
A) Pb + PbO2 + 2H2SO4 -> 2PbSO4 + 2H2O
B) PbSO4 + 2H2O -> Pb + PbO2 + 2H2SO4
C) Zn + Cu^2+ -> Zn^2+ + Cu
D) 2H2O -> 2H2 + O2
19. What is the main difference between a galvanic cell and an electrolytic cell?
A) Galvanic cells produce electricity, electrolytic cells consume it
B) Galvanic cells consume electricity, electrolytic cells produce it
C) Galvanic cells have a salt bridge, electrolytic cells do not
D) Galvanic cells use non-spontaneous reactions, electrolytic cells use spontaneous reactions
20. Which of the following is a characteristic of a primary cell?
A) It can be recharged
B) It is designed for a single use
C) It uses a reversible reaction
D) It has a high energy density
21. Faraday's second law of electrolysis states that if the same quantity of electricity is passed through different electrolytes, the masses of the substances liberated at the electrodes are proportional to their:
A) Atomic masses
B) Equivalent masses
C) Oxidation states
D) Electronegativities
22. What does the term 'overpotential' refer to in electrochemistry?
A) The potential required to overcome the activation energy of an electrode reaction
B) The potential difference across the electrolyte
C) The potential difference due to the salt bridge
D) The potential difference of the standard electrode
23. Which of the following is NOT a component of a Daniell cell?
A) Zinc electrode
B) Copper electrode
C) Sulphuric acid electrolyte
D) Salt bridge
24. The standard reduction potential for Cu^2+/Cu is +0.34 V. The standard oxidation potential for Cu/Cu^2+ is:
A) +0.34 V
B) -0.34 V
C) 0.00 V
D) +1.00 V
25. What is the function of an oxidant (oxidizing agent)?
A) To lose electrons
B) To gain electrons and cause oxidation
C) To lose electrons and cause reduction
D) To gain electrons and cause reduction
26. Which law states that the rate of reaction is proportional to the concentration of reactants?
A) Faraday's Law
B) Nernst Equation
C) Law of Mass Action
D) Ohm's Law
27. What is the oxidation state of sulfur in SO4^2-?
A) +4
B) +6
C) -2
D) -6
28. The flow of electrons in an external circuit of an electrochemical cell constitutes:
A) Ionic current
B) Electronic current
C) Displacement current
D) Induced current
29. Which type of cell produces electricity through a continuous supply of reactants?
A) Galvanic cell
B) Electrolytic cell
C) Fuel cell
D) Storage cell
30. What is the primary component of a battery?
A) A single electrochemical cell
B) A resistor
C) A capacitor
D) An inductor
31. In electroplating, the object to be plated is made the:
A) Anode
B) Cathode
C) Electrolyte
D) Power source
32. What is the unit of electrical resistance?
A) Siemens
B) Ohm
C) Volt
D) Faraday
33. Which substance is typically used to prevent corrosion?
A) Strong acids
B) Oxidizing agents
C) Protective coatings or sacrificial anodes
D) Reducing agents
34. Corrosion is an example of a spontaneous:
A) Electrolytic process
B) Redox reaction
C) Acid-base reaction
D) Precipitation reaction
35. In the electrolysis of molten NaCl, what product is formed at the cathode?
A) Cl2 gas
B) Na metal
C) H2 gas
D) O2 gas
36. What is the oxidation state of oxygen in most compounds?
A) +1
B) +2
C) -1
D) -2
37. Which of the following is a reducing agent?
A) O2
B) Cl2
C) H2
D) KMnO4
38. The cell potential (E_cell) can be calculated using the Nernst equation. If the reaction quotient (Q) is less than the equilibrium constant (K), then:
A) E_cell will be less than E°_cell
B) E_cell will be greater than E°_cell
C) E_cell will be equal to E°_cell
D) The reaction is at equilibrium
39. What is the purpose of a salt bridge in a galvanic cell?
A) To prevent the mixing of electrolytes
B) To complete the electrical circuit and maintain charge neutrality
C) To increase the cell potential
D) To provide a source of electrons
40. Which term describes the tendency of a substance to lose electrons?
A) Reduction potential
B) Oxidation potential
C) Electronegativity
D) Electron affinity
41. A spontaneous redox reaction occurs in a:
A) Electrolytic cell
B) Galvanic cell
C) Fuel cell
D) All of the above
42. What is the unit of electrical conductivity?
A) Ohm
B) Siemens per meter
C) Volt
D) Ampere
43. Faraday's first law of electrolysis states that the mass of a substance deposited at an electrode is proportional to the:
A) Electrode potential
B) Concentration of the electrolyte
C) Quantity of electricity passed
D) Temperature of the solution
44. Which of the following is a common application of electrolysis?
A) Battery charging
B) Rusting of iron
C) Photosynthesis
D) Combustion
45. What is the standard electrode potential of a standard hydrogen electrode (SHE) at 25°C?
A) +0.00 V
B) +1.00 V
C) -1.00 V
D) Undefined
46. In electrolysis, the electrode where reduction occurs is called the:
A) Anode
B) Cathode
C) Electrolyte
D) Terminal
47. What does the Nernst equation relate?
A) Cell potential to temperature
B) Cell potential to concentration
C) Reaction rate to concentration
D) Equilibrium constant to temperature
48. Which electrode in a galvanic cell is the site of oxidation?
A) Cathode
B) Anode
C) Salt Bridge
D) Electrolyte
49. What is the primary function of an electrolyte in an electrochemical cell?
A) To provide electrons
B) To conduct ions
C) To act as a catalyst
D) To absorb heat
50. In a redox reaction, what happens to the species that is oxidized?
A) It gains electrons
B) It loses electrons
C) Its oxidation state decreases
D) It acts as an oxidizing agent
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