Electrochemistry and Redox Reactions - One Line Questions

1. What is the standard electrode potential of a standard hydrogen electrode (SHE) at 25°C? — +0.00 V
2. The standard reduction potential for Cu^2+/Cu is +0.34 V. The standard oxidation potential for Cu/Cu^2+ is: — -0.34 V
3. What is the oxidation state of oxygen in most compounds? — -2
4. What is the oxidation state of nitrogen in HNO3? — +5
5. What is the oxidation state of sulfur in SO4^2-? — +6
6. What is the oxidation state of carbon in methane (CH4)? — -4
7. What is the primary component of a battery? — A single electrochemical cell
8. What is the unit of electrochemical potential difference? — Volt
9. In electroplating, the object to be plated is made the: — Cathode
10. In electrolysis, the electrode where reduction occurs is called the: — Cathode
11. 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: — Equivalent masses
12. Which of the following is a common application of electrolysis? — Battery charging
13. Which electrode in a galvanic cell is the site of oxidation? — Anode
14. The Nernst equation is derived from the relationship between Gibbs free energy change and: — Cell potential
15. What does the Nernst equation relate? — Cell potential to concentration
16. In the electrolysis of molten NaCl, what product is formed at the cathode? — Na metal
17. Which of the following metals has the lowest standard electrode potential and is thus the strongest reducing agent? — Lithium (Li)
18. What is the primary role of the Daniell cell in electrochemistry education? — Illustrating a spontaneous redox reaction generating electricity
19. 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: — E_cell will be greater than E°_cell
20. Faraday's first law of electrolysis states that the mass of a substance deposited at an electrode is proportional to the: — Quantity of electricity passed
21. Which process involves the direct conversion of chemical energy into electrical energy? — Galvanic Cell Operation
22. A spontaneous redox reaction occurs in a: — Galvanic cell
23. Corrosion is an example of a spontaneous: — Redox reaction
24. The process of depositing a thin layer of a desired metal onto another metal using electrolysis is called: — Electroplating
25. Which law states that the rate of reaction is proportional to the concentration of reactants? — Law of Mass Action
26. The rate of ionic migration in an electrolyte is proportional to the applied electric field strength. This is a consequence of: — Ohm's Law for electrolytes
27. Which type of cell produces electricity through a continuous supply of reactants? — Fuel cell
28. What is the main difference between a galvanic cell and an electrolytic cell? — Galvanic cells produce electricity, electrolytic cells consume it
29. The flow of electrons in an external circuit of an electrochemical cell constitutes: — Electronic current
30. Which of the following is a characteristic of a primary cell? — It is designed for a single use
31. What happens to the anode in a typical galvanic cell made of two different metals and their salt solutions? — It dissolves and loses mass
32. In a redox reaction, what happens to the species that is oxidized? — It loses electrons
33. Which phenomenon is responsible for the rusting of iron? — Electrochemical corrosion
34. Which of the following is a reducing agent? — H2
35. The unit of electrical conductance is: — Siemens
36. What is the unit of electrical conductivity? — Siemens per meter
37. What is the overall reaction in a lead-acid battery during discharge? — Pb + PbO2 + 2H2SO4 -> 2PbSO4 + 2H2O
38. Which of the following is an example of an electrolytic refining process? — Purification of copper
39. Which of the following is a strong electrolyte? — Dilute sulfuric acid
40. In a fuel cell, the reactants are supplied externally and continuously, while the products are removed. This allows for: — Continuous operation
41. Which term describes the tendency of a substance to lose electrons? — Oxidation potential
42. What is the unit of electrical resistance? — Ohm
43. Which substance is typically used to prevent corrosion? — Protective coatings or sacrificial anodes
44. What is the standard cell potential (E°_cell) of a galvanic cell? — The potential difference under standard conditions (1 M concentration, 1 atm pressure, 25°C)
45. What does the term 'overpotential' refer to in electrochemistry? — The potential required to overcome the activation energy of an electrode reaction
46. Electrochemical impedance spectroscopy (EIS) is a technique used to study: — The electrical properties of electrochemical interfaces
47. What is the function of an oxidant (oxidizing agent)? — To gain electrons and cause reduction
48. What is the purpose of a salt bridge in a galvanic cell? — To complete the electrical circuit and maintain charge neutrality
49. What is the primary function of an electrolyte in an electrochemical cell? — To conduct ions
50. Which of the following is a unit of electric charge? — Coulomb
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