This quiz works best with JavaScript enabled. Home > Cbse > Class 12 > Science > Chemistry Part I > Class 12 Chemistry (Part I) Chapter 3 Electrochemistry – Quiz 5 🏠 Homepage 📘 Download PDF Books 📕 Premium PDF Books Class 12 Chemistry (Part I) Chapter 3 Electrochemistry Quiz 5 (60 MCQs) Quiz Instructions Select an option to see the correct answer instantly. 1. Which of the following is true about an electrolyte?I Electrolyte conducts electricity in molten state.II Electrolyte conducts electricity in solid state.III Electrolyte is soluble in water.IV Electrolyte undergoes chemical decomposition when it conducts electricity. A) I and II only. B) II and III only. C) II and IV only. D) I and IV only. Show Answer Correct Answer: D) I and IV only. 2. Silver chloride can conduct electrocity in molten state, but not conducting in solid state. This is because silver chloride A) Has freely moving electrons in molten state. B) Exist as atoms in solid state. C) Exist as freely moving charged particles in molten state. D) Is a covalent compound. Show Answer Correct Answer: C) Exist as freely moving charged particles in molten state. 3. The correct relation between Avogadro's number and Faraday's constant is: A) F= WIt/E. B) W= EIt/F. C) F= WItE. D) W= FIt/E. Show Answer Correct Answer: B) W= EIt/F. 4. Consider the following half equation:Br$_{2}$(l) + 2e$^{-}$ $\rightarrow$ 2Br$^{-}$ (aq) E$^{0}$ = +1.07 VFe$^{2+}$ (aq) + 2e$^{-}$ $\rightarrow$ Fe(s) E$^{0}$ =-0.44 Vwhich of the following is a correct statement. A) Fe is a stronger reducing agent than Br$_{2}$. B) Fe is a stronger reducing agent than Br$^{-}$. C) Fe$^{2+}$ is a stronger reducing agent than Br$^{-}$. D) Fe is stronger reducing agent than Fe$^{2+}$. Show Answer Correct Answer: B) Fe is a stronger reducing agent than Br$^{-}$. 5. Electrical energy is produced in a voltaic cell by a ..... redox reaction within the cell. A) Nonspontaneous. B) Spontaneous. C) All the above. D) None of the above. Show Answer Correct Answer: B) Spontaneous. 6. Compare and contrast the functions of the anode and cathode in electrochemical cells. A) The anode and cathode both accept electrons through reduction. B) The anode accepts electrons through reduction, while the cathode releases electrons through oxidation. C) The anode releases electrons through oxidation, while the cathode accepts electrons through reduction. D) The anode and cathode both release electrons through oxidation. Show Answer Correct Answer: C) The anode releases electrons through oxidation, while the cathode accepts electrons through reduction. 7. Which electrode in a galvanic cell is positive? A) Anode. B) Cathode. C) Both are equally positive. D) Neither, as they are both neutral. Show Answer Correct Answer: B) Cathode. 8. In a concentration cell, how does the Nernst equation explain the generation of voltage? A) Voltage is generated by the presence of a catalyst. B) Voltage is generated by the temperature difference between electrodes. C) Voltage is generated due to the concentration gradient between two half-cells. D) Voltage is generated by the pressure difference in the cell. Show Answer Correct Answer: C) Voltage is generated due to the concentration gradient between two half-cells. 9. Which change occurs at the anode in an operating electrochemical cell? A) Loss of electrons. B) Gain of electrons. C) Gain of protons. D) Loss of protons. Show Answer Correct Answer: A) Loss of electrons. 10. What is the role of a cathode and anode in electrochemical reactions? A) The anode is where reduction occurs and gains electrons. B) The anode is where oxidation occurs and loses electrons, while the cathode is where reduction occurs and gains electrons. C) Both the anode and cathode are sites of oxidation. D) The anode gains electrons while the cathode loses electrons. Show Answer Correct Answer: B) The anode is where oxidation occurs and loses electrons, while the cathode is where reduction occurs and gains electrons. 11. Which of the following is a real-world application of electrochemistry? A) Photosynthesis in plants. B) Combustion engines. C) Batteries and fuel cells. D) Nuclear reactors. Show Answer Correct Answer: C) Batteries and fuel cells. 12. List some common applications of electrochemistry in daily life. A) Hydraulic systems. B) Wind turbines. C) Batteries, electroplating, corrosion prevention, electrolysis. D) Solar panels. Show Answer Correct Answer: C) Batteries, electroplating, corrosion prevention, electrolysis. 13. What is electrode potential? A) Electrode potential is the measure of the color of an electrode. B) Electrode potential is the measure of the tendency of an electrode to gain or lose electrons in contact with a solution of its own ions. C) Electrode potential is the measure of the amount of ions in an electrode when in contact with a solution of its own ions. D) Electrode potential is the measure of the temperature of an electrode. Show Answer Correct Answer: B) Electrode potential is the measure of the tendency of an electrode to gain or lose electrons in contact with a solution of its own ions. 14. In a galvanic cell, which component is responsible for the flow of electrons? A) Cathode. B) Salt bridge. C) Electrolyte solution. D) Anode. Show Answer Correct Answer: A) Cathode. 15. Electronic conduction is due to flow of A) Electrons. B) Protons. C) Ions. D) Neutrons. Show Answer Correct Answer: A) Electrons. 16. What are redox reactions and how do they occur? A) Redox reactions do not involve any changes in oxidation states. B) Redox reactions are chemical reactions where one substance is oxidized and another is reduced, involving the transfer of electrons. C) Redox reactions are limited to reactions in acidic solutions only. D) Redox reactions only involve the formation of new compounds without electron transfer. Show Answer Correct Answer: B) Redox reactions are chemical reactions where one substance is oxidized and another is reduced, involving the transfer of electrons. 17. The difference between the electrode potentials of two electrodes when no current is drawn through the cell is called ..... A) Cell potential. B) Potential difference. C) Cell emf. D) Cell voltage. Show Answer Correct Answer: C) Cell emf. 18. Which of the following is a primary cell? A) Lithium-ion battery. B) Nickel-cadmium battery. C) Dry cell. D) Lead-acid battery. Show Answer Correct Answer: C) Dry cell. 19. Because copper is not easily oxidized, it is often used as the ..... in voltaic cells. A) Ion. B) Electrolyte bridge. C) Anode. D) Cathode. Show Answer Correct Answer: D) Cathode. 20. The half-reaction that occurs at the anode during the electrolysis of molten sodium bromide is? A) Na $\rightarrow$ Na$^{+}$ + e$^{-}$. B) 2 Br$^{-}$$\rightarrow$ Br$_{2}$ + 2 e$^{-}$. C) Br$_{2}$ + 2 e$^{-}$ $\rightarrow$ 2 Br$^{-}$. D) Na$^{+}$ + e$^{-}$ $\rightarrow$ Na. Show Answer Correct Answer: B) 2 Br$^{-}$$\rightarrow$ Br$_{2}$ + 2 e$^{-}$. 21. Which of the following is true for an electrolytic cell? A) Changes electrical energy into chemical energy. B) Used in electroplating. C) Uses an electricity to make a nonspontaneous reaction go. D) All of the above. Show Answer Correct Answer: D) All of the above. 22. Also known as or ion bridge, in electrochemistry, is a laboratory device used to connect the oxidation and reduction half-cells of a galvanic cell (voltaic cell). A) Galvanic bridge. B) Salt bridge. C) Voltaic bridge. D) Electrochemical bridge. Show Answer Correct Answer: B) Salt bridge. 23. Chemical cells produce a voltage. When do they stop producing a voltage and 'go flat'? A) When one of the reactants has run out. B) When they get too hot. C) When they reach the expiry date on the cell. D) None of the above. Show Answer Correct Answer: A) When one of the reactants has run out. 24. In a chemical cell, chemical energy change to ..... energy A) Electrical. B) Chemical. C) All the above. D) None of the above. Show Answer Correct Answer: A) Electrical. 25. A redox reaction has an equilibrium constant of K = 2.6 x 10$^{5}$. Which of the following statements best represents the algebraic signs of E$^{o}$$_{cell}$ and G$^{o}$$_{rxn}$ for this reaction? A) E$^{o}$$_{cell}$ is positive and G$^{o}$$_{rxn}$ is positive. B) E$^{o}$$_{cell}$ is negative and G$^{o}$$_{rxn}$ is negative. C) E$^{o}$$_{cell}$ is positive and G$^{o}$$_{rxn}$ is negative. D) E$^{o}$$_{cell}$ is negative and G$^{o}$$_{rxn}$ is positive. Show Answer Correct Answer: C) E$^{o}$$_{cell}$ is positive and G$^{o}$$_{rxn}$ is negative. 26. M(s) + 3Ag$^{+}$(aq) $\rightarrow$3Ag(s) + M$^{3+}$(aq)$^{ }$E$^\circ$ = +2.46 VAg$^{+}$(aq) + e$^{-}$$\rightarrow$Ag(s) E$^\circ$ = +0.80 VAccording to the information above, what is the standard reduction potential for the half-reaction M$^{3+}$(aq) + 3e$^{-}$$\rightarrow$M(s)? A) -1.66 V. B) 1.66 V. C) 0.06 V. D) -0.06 V. Show Answer Correct Answer: A) -1.66 V. 27. In a Galvanic cell, the electrons flow from the ..... A) Anode to the cathode. B) Cathode to the anode. C) All the above. D) None of the above. Show Answer Correct Answer: A) Anode to the cathode. 28. An aqueous solution of CuSO$_{4}$ is electrolysedusing a current of 0.150 A for 5 hours. Calculate the mass of copper deposited at cathode.(Molar mass of Cu = 63.6 g/mol) A) 0.0140 g. B) 1.7794 g. C) 0.8897 g. D) 0.4449 g. Show Answer Correct Answer: C) 0.8897 g. 29. What is the significance of electron flow control in electrochemical systems? A) It increases the temperature of the system. B) It allows for the storage and release of energy efficiently. C) It changes the color of the reactants. D) It decreases the pressure within the system. Show Answer Correct Answer: B) It allows for the storage and release of energy efficiently. 30. Which process is used to drive non-spontaneous reactions in electrochemistry? A) Galvanization. B) Combustion. C) Fermentation. D) Electrolysis. Show Answer Correct Answer: D) Electrolysis. 31. The element that usually does NOT show variable oxidation states is: A) Cu. B) Ti. C) Sc. D) V. Show Answer Correct Answer: C) Sc. 32. When an electrochemical cell is operating, it is A) Approaching equilibrium. B) Undergoing reduction, only. C) Using external energy. D) Undergoing oxidation, only. Show Answer Correct Answer: A) Approaching equilibrium. 33. Describe the process of corrosion and its effects. A) Corrosion only affects non-metal materials like plastics. B) Corrosion is the deterioration of materials, especially metals, due to chemical reactions with their environment, leading to structural damage and material loss. C) Corrosion is a method of enhancing the durability of metals. D) Corrosion is a process that strengthens metals against wear. Show Answer Correct Answer: B) Corrosion is the deterioration of materials, especially metals, due to chemical reactions with their environment, leading to structural damage and material loss. 34. Which of the is the oxidation half reaction for the following redox reaction?Cu + 2 AgNO$_{3}$ $\rightarrow$ Cu(NO$_{3}$)$_{2}$ + 2 Ag A) Ag$^{+}$ $\rightarrow$ Ag + 2 e$^{-}$. B) Cu $\rightarrow$ Cu$^{2+}$ + 2 e$^{-}$. C) Cu + 2 e$^{-}$ $\rightarrow$ Cu$^{2+}$. D) Ag$^{+}$ + e$^{-}$ $\rightarrow$ Ag. Show Answer Correct Answer: B) Cu $\rightarrow$ Cu$^{2+}$ + 2 e$^{-}$. 35. In coordination compounds, the ligands act as A) Lewis acid. B) Arrhenius base. C) Arrhenius acid. D) Lewis base. Show Answer Correct Answer: D) Lewis base. 36. Electrons are gained at the A) Anode. B) Cathode. C) All the above. D) None of the above. Show Answer Correct Answer: B) Cathode. 37. Salinity favors corrosion. A) True. B) False. C) All the above. D) None of the above. Show Answer Correct Answer: A) True. 38. Which half-reaction equation represents reduction? A) Cu$\rightarrow$ Cu$^{+2}$+2e. B) Ag$^{+}$$\rightarrow$ Ag + e. C) Cu$^{+2}$+2e $\rightarrow$ Cu. D) Ag +. e $\rightarrow$ Ag$^{+}$. Show Answer Correct Answer: C) Cu$^{+2}$+2e $\rightarrow$ Cu. 39. A group of voltaic cells connected together. A) Dry cells. B) Lead storage batteries. C) Fuel cells. D) None of the above. Show Answer Correct Answer: B) Lead storage batteries. 40. What are the ions present in molten lead (II) bromide? A) PbBr$_{2}$. B) Pb and Br. C) Pb$^{2+}$ and Br$^{-}$. D) Pb$^{2+}$ and Br$_{2}$$^{-}$. Show Answer Correct Answer: C) Pb$^{2+}$ and Br$^{-}$. 41. The anode is where A) Electrolyte concentrations are lowest. B) Oxidation occurs. C) Anions are produced. D) Electrolyte concentrations are highest. Show Answer Correct Answer: B) Oxidation occurs. 42. Which features does a standard hydrogen electrode have?I. A temperature of 298 KII. A carbon electrodeIII. Hydrogen gas at 1.01x 10$^{5}$ Pa (1 atm) pressure A) I and II. B) I and III. C) II and III. D) I, II and III. Show Answer Correct Answer: B) I and III. 43. How does the flow of electrons occur in an electrochemical cell? A) Electrons flow from the cathode to the anode through an external circuit. B) Electrons flow from the cathode to the anode through the electrolyte. C) Electrons flow from the anode to the cathode through the electrolyte. D) Electrons flow from the anode to the cathode through an external circuit. Show Answer Correct Answer: D) Electrons flow from the anode to the cathode through an external circuit. 44. WHAT BEST DESCRIBES GALVANIC CELL? A) A GALVANIZED PRISON CELL. B) CHICKEN TIKKA. C) PRODUCES ELECTRICITY VIA A CHEMICAL REACTION. D) CHEMICAL REACTION INITIATED BY A FLOW OF CURRENT. Show Answer Correct Answer: C) PRODUCES ELECTRICITY VIA A CHEMICAL REACTION. 45. How is the cell potential of a galvanic cell calculated? A) By adding the reduction potentials of the anode and cathode. B) By subtracting the anode potential from the cathode potential. C) By multiplying the standard reduction potentials of the half-cells. D) By dividing the anode potential by the cathode potential. Show Answer Correct Answer: B) By subtracting the anode potential from the cathode potential. 46. In the context of electrochemistry, what does the term "cell potential" refer to? A) The potential energy of the cell's components. B) The capacity of the cell to store charge. C) The maximum current the cell can produce. D) The electrical potential difference between the two electrodes. Show Answer Correct Answer: D) The electrical potential difference between the two electrodes. 47. Which is correct to write cell notation Anode:ZnCathode:Ni A) Zn$^{2+ }$(s, 1M) / Zn (aq) // Ni (aq) / Ni$^{2+ }$(s, 1M). B) Zn$^{2+ }$(aq, 1M) / Zn (s) // Ni (s) / Ni$^{2+ }$(aq, 1M). C) Zn (aq) /Zn$^{2+ }$(s, 1M) // Ni$^{2+ }$(s, 1M) / Ni (aq). D) Zn (s) /Zn$^{2+ }$(aq, 1M) // Ni$^{2+ }$(aq, 1M) / Ni (s). Show Answer Correct Answer: D) Zn (s) /Zn$^{2+ }$(aq, 1M) // Ni$^{2+ }$(aq, 1M) / Ni (s). 48. What is the main function of an electrolyte in an electrochemical cell? A) To increase the cell voltage. B) To provide a source of ions for the reaction. C) To provide a medium for electron flow. D) To prevent the flow of electrons. Show Answer Correct Answer: B) To provide a source of ions for the reaction. 49. The standard potential of hydrogen electrode at 1M concentration and hydrogen gas at 1 atm pressure is A) 1V. B) 0V. C) 6V. D) 8V. Show Answer Correct Answer: B) 0V. 50. This electrode in a voltaic cell gains mass A) Anode. B) Cathode. C) All the above. D) None of the above. Show Answer Correct Answer: B) Cathode. 51. What kind of electric cell are we going to be working with in this lab? A) Anode. B) Voltaic. C) Cathode. D) Electrolytic. Show Answer Correct Answer: B) Voltaic. 52. Katod bagi sel kimia ialah A) Elektrod negatif. B) Elektrod positif. C) Ion bercas positif. D) Ion bercas negatif. Show Answer Correct Answer: B) Elektrod positif. 53. 3 Faraday's of electricity is passed through Al2O3, CuSO4 and NaCl taken in three electrolytic cells. The amount of Al, Cu and Na deposited at the cathode will be in the ratio A) 1 mole:1.5 mole:3 mole. B) 3 mole:1 mole:2 mole. C) 1 mole:2 mole:3 mole. D) 1.5 mole:2 mole:3 mole. Show Answer Correct Answer: A) 1 mole:1.5 mole:3 mole. 54. How is the standard electrode potential measured? A) The standard electrode potential is measured using a galvanic cell with a standard hydrogen electrode. B) By measuring the temperature of the solution. C) Using a voltmeter directly on the electrode. D) Through a spectroscopic analysis of the electrode. Show Answer Correct Answer: A) The standard electrode potential is measured using a galvanic cell with a standard hydrogen electrode. 55. How much charge in Faraday is required for the following reductions:1 mol of Al3+ to Al. A) 4F. B) 2F. C) 1F. D) 3F. Show Answer Correct Answer: D) 3F. 56. Are dry cell batteries one example of galvanic cells? A) True. B) False. C) All the above. D) None of the above. Show Answer Correct Answer: A) True. 57. Dilute aqueous zinc chloride is electrolysed using platinum electrodes. What are the products at the electrodes? A) Cathode:zinccathode:oxygen. B) Anode:hydrogencathode:oxygen. C) Anode:oxygencathode:hydrogen. D) Anode:chlorinecathode:hydrogen. Show Answer Correct Answer: C) Anode:oxygencathode:hydrogen. 58. In weak electrolytes, ..... dissociation of ions takesplace. A) Complete. B) Half. C) 25%. D) Partial. Show Answer Correct Answer: D) Partial. 59. Which of the following compounds is widely used as a breath analyzer? A) Potassium dichromate. B) Potassium permanganate. C) Potassium chloride. D) Potassium sulfate. Show Answer Correct Answer: A) Potassium dichromate. 60. Ion yang bercas negatif A) Kation. B) Anod. C) Anion. D) Katod. Show Answer Correct Answer: C) Anion. ← PreviousNext →Related QuizzesScience QuizzesClass 12 QuizzesClass 12 Chemistry (Part I) Chapter 3 Electrochemistry Quiz 1Class 12 Chemistry (Part I) Chapter 3 Electrochemistry Quiz 2Class 12 Chemistry (Part I) Chapter 3 Electrochemistry Quiz 3Class 12 Chemistry (Part I) Chapter 3 Electrochemistry Quiz 4Class 12 Chemistry (Part I) Chapter 3 Electrochemistry Quiz 6Class 12 Chemistry (Part I) Chapter 3 Electrochemistry Quiz 7Class 12 Chemistry (Part I) Chapter 3 Electrochemistry Quiz 8Class 12 Chemistry (Part I) Chapter 3 Electrochemistry Quiz 9 🏠 Back to Homepage 📘 Download PDF Books 📕 Premium PDF Books