This quiz works best with JavaScript enabled. Home > Cbse > Class 12 > Science > Chemistry Part I > Class 12 Chemistry (Part I) Chapter 3 Electrochemistry – Quiz 4 🏠 Homepage 📘 Download PDF Books 📕 Premium PDF Books Class 12 Chemistry (Part I) Chapter 3 Electrochemistry Quiz 4 (60 MCQs) Quiz Instructions Select an option to see the correct answer instantly. 1. Calculate the electrode potential of a copper wire dipped in 0.1M CuSO$_{4}$ solution at 25$^{o}$C . The standard electrode potential of copper is 0.34 V . A) 0.2809 V. B) 3.1045 V. C) 2.809 V. D) 0.31045 V. Show Answer Correct Answer: D) 0.31045 V. 2. The charge required for the reduction of 1 mol of MnO$_{4}$$^{-}$to MnO$_{2}$ is A) 6 F. B) 1 F. C) 5 F. D) 3 F. Show Answer Correct Answer: D) 3 F. 3. In electrolytic cells, the external power source is used to: A) Measure the cell potential. B) Drive a non-spontaneous chemical reaction. C) Cool down the electrolyte solution. D) Increase the concentration of the electrolyte. Show Answer Correct Answer: B) Drive a non-spontaneous chemical reaction. 4. The electrolysis of brine produces A) Water, sodium metal and chlorine gas. B) Aqueous sodium hydroxide, hydrogen gas and chlorine gas. C) Sodium metal and hydrogen gas. D) Hydrochloric acid and sodium metal. Show Answer Correct Answer: B) Aqueous sodium hydroxide, hydrogen gas and chlorine gas. 5. The species oxidized in corrosion A) Fe. B) O$_{2}$. C) Mg. D) None of the above. Show Answer Correct Answer: A) Fe. 6. Assume that the following reaction proceeds in an electrolytic cell. If 1.5A of current are used for 2.0 hours, what will plate and how many grams are expected?Fe$^{+2}$ (aq) + Ni (s) $\rightarrow$ Fe (s) + Ni$^{+2}$ (aq) A) Nickel plates; 9.1 x 10$^{-4}$grams. B) Iron plates; 3.1 grams. C) Nickel plates; 3.3 grams. D) Iron plates; 8.7 x 10$^{-4}$ grams. Show Answer Correct Answer: B) Iron plates; 3.1 grams. 7. What does the voltage of a cell depend on? A) The size of the cell. B) How much oxygen is present. C) The difference in reactivity of the two electrodes. D) None of the above. Show Answer Correct Answer: C) The difference in reactivity of the two electrodes. 8. Which metal will spontaneously react with Zn$^{2+}$(aq), but will not spontaneously react with Mg$^{2+}$(aq)? A) Cu. B) Ba. C) Ni. D) Mn. Show Answer Correct Answer: D) Mn. 9. What is the purpose of the salt bridge in electrolytic cells? A) Electrolytic cells do not use a salt bridge. B) To supply additional electrolytes. C) To generate electricity. D) To prevent the electrodes from touching. Show Answer Correct Answer: A) Electrolytic cells do not use a salt bridge. 10. What are the products of electrolysis of water? A) Hydrogen and Oxygen. B) Sodium and Chlorine. C) Hydrogen Peroxide and Methane. D) Nitrogen and Carbon Dioxide. Show Answer Correct Answer: A) Hydrogen and Oxygen. 11. Calculate E for the following electrochemical cell at 25$^\circ$CPt | H$_{2}$(g) (1.0 atm) | H$^{+}$ (0.010 M) || Ag$^{+}$ (0.020 M) | Agif E$^\circ$ (H$^{+}$) = +0.000 V and E$^\circ$ (Ag$^{+}$) = 0.799 V A) +0.275 V. B) +0.911 V. C) +0.817 V. D) +0.799 V. Show Answer Correct Answer: B) +0.911 V. 12. Terminal positif sel elektrolisis A) Anod. B) Anion. C) Katod. D) Kation. Show Answer Correct Answer: A) Anod. 13. The molar conductivity of a 0.5 mol/dm$^{3}$ solution of AgNO3 with specific conductance of 5.76 x 10$^{-3}$ S cm$^{-1}$ at 298 K is A) 11.52 S cm$^{2}$/ mol. B) 28.8 S cm$^{2}$/ mol. C) 0.086 S cm$^{2}$/ mol. D) 2.88 S cm$^{2}$/ mol. Show Answer Correct Answer: A) 11.52 S cm$^{2}$/ mol. 14. Which of the following statements is(are) true for all voltaic (or galvanic) cells?(I) Reduction occurs at the cathode(II) The anode gains mass during discharge (note:this means operation of the cell.)(III) The voltage is less than or equal to zero. A) Only III. B) II and III. C) Only II. D) Only I. Show Answer Correct Answer: D) Only I. 15. What is the Nernst equation used for in electrochemistry? A) To calculate the equilibrium constant of a reaction. B) To determine the cell potential under non-standard conditions. C) To measure the pH of a solution. D) To find the concentration of ions in a solution. Show Answer Correct Answer: B) To determine the cell potential under non-standard conditions. 16. What occurs to the mass of zinc electrode in the following reaction?Zn/Zn+2 // Ag+1 / Ag A) Increases. B) Decreases. C) Remains the same. D) None of the above. Show Answer Correct Answer: B) Decreases. 17. How does the Nernst equation relate to concentration cells? A) It shows that cell potential is independent of concentration. B) It indicates that cell potential is directly proportional to concentration. C) It explains how cell potential varies with concentration differences. D) It demonstrates that cell potential is inversely proportional to concentration. Show Answer Correct Answer: C) It explains how cell potential varies with concentration differences. 18. Reactions in electrolytic cells are A) Non-spontaneous, non-redox reactions. B) Spontaneous, redox reactions. C) Non-spontaneous, redox reactions. D) Spontaneous, non-redox reactions. Show Answer Correct Answer: C) Non-spontaneous, redox reactions. 19. What factors influence the rate of electrolysis? A) Humidity levels in the environment. B) Type of light used during the process. C) Presence of magnetic fields. D) Factors influencing the rate of electrolysis include electrolyte type, concentration, temperature, electrode surface area, applied voltage, and electrode material. Show Answer Correct Answer: D) Factors influencing the rate of electrolysis include electrolyte type, concentration, temperature, electrode surface area, applied voltage, and electrode material. 20. If a conductivity and conductance of a solution is same then it's cell constant A) 10. B) 1000. C) 1. D) 0. Show Answer Correct Answer: C) 1. 21. Standard Conditions Galvanic Cells would be A) 1.0 M solutions. B) 1 atm pressure. C) 25$^{o}$ Celsius. D) All of the above. Show Answer Correct Answer: D) All of the above. 22. Specific conductance decreases with A) Decrese in concentration. B) Increse in concentration. C) Remains constant. D) None. Show Answer Correct Answer: A) Decrese in concentration. 23. In electrolytic cells, the cathode is characterized by: A) Neutralization. B) Precipitation. C) Reduction. D) Oxidation. Show Answer Correct Answer: C) Reduction. 24. The efficiency of a salt bridge is primarily due to its ability to: A) Increase the voltage of the cell. B) Maintain the charge balance by ion exchange. C) Store excess energy produced by the cell. D) Conduct electrons between the half-cells. Show Answer Correct Answer: B) Maintain the charge balance by ion exchange. 25. Which of the following reactions shows that copper is oxidized? A) Reaction of magnesium with copper (II)oxide. B) Reaction of copper with silver nitrate solution. C) Electrolysis of copper (II) nitratesolution by using carbon nitrate. D) Voltaic cell with copper and magnesiumelectrodes in dilute sulphuric acid. Show Answer Correct Answer: B) Reaction of copper with silver nitrate solution. 26. Which atom forms an ion that would migrate toward the cathode in an electrolytic cell? A) Na. B) I. C) F. D) Cl. Show Answer Correct Answer: A) Na. 27. Which of the following substances does not conduct electricity? A) Crystalline NaCl. B) Graphite. C) CuSO4 solution. D) NaCl crystals with a defect. Show Answer Correct Answer: A) Crystalline NaCl. 28. Why electrolytes in the solid state cannot conduct electricity? A) Solid state needs current with a high voltage. B) Solid state has a fixed volume. C) Solid state does not have free-moving ions. D) Solid state has a fixed shape. Show Answer Correct Answer: C) Solid state does not have free-moving ions. 29. How is voltage related to Gibbs free energy in electrochemical reactions? A) Voltage is equal to Gibbs free energy. B) Voltage is directly proportional to Gibbs free energy. C) Voltage is inversely proportional to Gibbs free energy. D) Voltage is unrelated to Gibbs free energy. Show Answer Correct Answer: B) Voltage is directly proportional to Gibbs free energy. 30. How many moles of aluminum metal can be deposited when 0.600 moles of electrons are passed through 4.00 moles of molten Al$_{2}$O$_{3}$? A) 0.200. B) 0.100. C) 1.80. D) 1.33. Show Answer Correct Answer: A) 0.200. 31. In the galvanic cell in which the reaction Zn(s)+2Ag+(aq) $\rightarrow$Zn2+(aq)+2Ag(s)takes place. (i) Which of the electrode is negatively charged? A) Zn. B) Cathode. C) Salt bridge. D) Ag. Show Answer Correct Answer: A) Zn. 32. The cathode is known as the ..... half of the cell. A) Inactive. B) Negative. C) Neutral. D) Positive. Show Answer Correct Answer: D) Positive. 33. In a Galvanic/Voltaic Cell, the salt bridge ..... A) Completes the circuit so that electrons can flow through the wire. B) Maintains electrical neutrality. C) Avoid liquid junction potential. D) All of the above. Show Answer Correct Answer: D) All of the above. 34. Fill in the blank."In the Hydrogen electrode, the electrode is placed in a solution of ..... M HCl." A) 3. B) 1. C) 0.5. D) 2. Show Answer Correct Answer: B) 1. 35. Standard electrode potential of a half-cell is measured with reference to A) Standard hydrogen electrode with 0.500M [HCl] solution. B) Standard oxygen electrode with 1.00M [HCl] solution. C) Standard chlorine electrode with 1.00M [HCl] solution. D) Standard hydrogen electrode with 1.00 M [HCl] solution. Show Answer Correct Answer: D) Standard hydrogen electrode with 1.00 M [HCl] solution. 36. Which of the following pairs can produce the highest reading on the voltmeter? A) Magnesium / Silver. B) Magnesium / Copper. C) Zinc / Magnesium. D) Zinc / Copper. Show Answer Correct Answer: A) Magnesium / Silver. 37. A chemical species in an electrochemical reaction that GAINS electrons undergoes ..... A) Oxidation Reaction. B) Reduction Reaction. C) All the above. D) None of the above. Show Answer Correct Answer: B) Reduction Reaction. 38. When a Mg atom becomes a Mg$^{2+}$ ion, the number of protons in the nucleus A) Increases. B) Decreases. C) Stays the same. D) None of the above. Show Answer Correct Answer: C) Stays the same. 39. Electrical energy is converted to Chemical energy in ..... A) A chemical Cell. B) An Electrolytic Cell. C) All the above. D) None of the above. Show Answer Correct Answer: B) An Electrolytic Cell. 40. In which substance does chlorine have an oxidation number of +1? A) HCl. B) Cl$_{2}$. C) HClO$_{2}$. D) HClO. Show Answer Correct Answer: D) HClO. 41. A positive ion is called a(n) ..... , while a negative ion is called a(n) ..... A) Anion, cation. B) Cation, anion. C) Oxidation, reduction. D) Isotope, ion. Show Answer Correct Answer: B) Cation, anion. 42. Uses electrical energy to pump electrons. A) Electrochemical cell. B) Galvanic cell. C) Voltaic cell. D) Electrolytic cell. Show Answer Correct Answer: D) Electrolytic cell. 43. In which direction does electricity flow in a voltaic cell (battery)? A) Electrons flow from right to left. B) Electrons flow from left to right. C) Electrons flow from anode to cathode. D) Electrons flow from the cathode to the anode. Show Answer Correct Answer: C) Electrons flow from anode to cathode. 44. In a galvanic cell, what is the role of the anode? A) It is where oxidation occurs. B) It is where reduction occurs. C) It is the site of electron gain. D) It is the site of ion exchange. Show Answer Correct Answer: A) It is where oxidation occurs. 45. If limiting molar conductivity of Ca2+ and Cl-are 119.0 and 76.3 S cm2 mol-1, then the value of limiting molar conductivity of CaCl2 will be A) 43.3 S cm2 mol-1. B) 195.3 S cm2 mol-1. C) 314.3 S cm2 mol-1. D) 271.6 S cm2 mol-1. Show Answer Correct Answer: D) 271.6 S cm2 mol-1. 46. Determine the values of $\Delta$G$^\circ$ for the following reaction:Ni$_{(s)}$ + 2Ag$^{+}$$_{ (aq)}$ $\rightarrow$ Ni$^{2+}$ $_{(aq)}$ + 2Ag$_{(s)}$, E$^\circ$ = 1.05 V(1F = 96500 C mol$^{-1}$) A) $\Delta$G$^\circ$ = 232.65 KJ mol$^{-1}$. B) $\Delta$G$^\circ$ =-202.65 KJ mol$^{-1}$. C) $\Delta$G$^\circ$ =-102.65 KJ mol$^{-1}$. D) $\Delta$G$^\circ$ =-242.65 KJ mol$^{-1}$. Show Answer Correct Answer: B) $\Delta$G$^\circ$ =-202.65 KJ mol$^{-1}$. 47. Where can hydrogen be obtained from on the space station without transporting it from Earth? A) From plants. B) From water. C) From the Moon. D) None of the above. Show Answer Correct Answer: B) From water. 48. An example of an anion is ..... A) $K^+$. B) $Cl^-$. C) $Na^+$. D) $Na^+$. Show Answer Correct Answer: B) $Cl^-$. 49. With increase in dilution the conductivity increases. A) TRUE. B) FALSE. C) All the above. D) None of the above. Show Answer Correct Answer: B) FALSE. 50. Mg + PbCl$_{2}$ $\rightarrow$ MgCl$_{2}$ + PbWhich statement correctly describes the oxidation and reduction that occur? A) Mg is oxidized and Pb$^{+2}$ is reduced. B) Mg is oxidized and Cl$^{-}$ is reduced. C) Mg is reduced and Cl$^{-}$ is oxidized. D) Mg is reduced and Pb$^{+2}$ is oxidized. Show Answer Correct Answer: A) Mg is oxidized and Pb$^{+2}$ is reduced. 51. An electrolytic cell uses electrical energy to drive A) A biological reaction. B) A non-spontaneous chemical reaction. C) A spontaneous chemical reaction. D) A physical change. Show Answer Correct Answer: B) A non-spontaneous chemical reaction. 52. Given the standard reduction potentials, Eo of iron is-0.44V and Eo of oxygen is 1.23V.what will be the emf of the cell? A) -0.79V. B) -1.67V. C) 1.67V. D) 0.79V. Show Answer Correct Answer: C) 1.67V. 53. Which one can be recharged A) Mercury cell. B) Lead storage battery. C) Lechlenche cell. D) All of these. Show Answer Correct Answer: B) Lead storage battery. 54. Determine the $\Delta$G, use F= 96458 J/V mol e-:-0.311 V, n = 3 A) 89.995 kJ/mol. B) 91 kJ/mol. C) 89.980 kJ/mol. D) 89.994 kJ/mol. Show Answer Correct Answer: A) 89.995 kJ/mol. 55. Define corrosion. A) Corrosion is the process of conversion of a metal into undesirable compounds on exposure to the atmosphere. B) Corrosion is the process of preserving a material by exposing it to chemicals. C) Corrosion is the process of strengthening a material through chemical reactions. D) Corrosion is the process of cleaning a material using chemical reactions. Show Answer Correct Answer: A) Corrosion is the process of conversion of a metal into undesirable compounds on exposure to the atmosphere. 56. How much electricity in terms of Faradays is required to produce 20 g of calcium from molten CaCl$_{2}$? [Molar mass of Ca is 40] A) 2F. B) 3F. C) 1F. D) None of the above. Show Answer Correct Answer: C) 1F. 57. In the reaction:Fe + Cu$^{2+ }$ $\rightarrow$Fe$^{2+}$ + CuWhat is your anode electrode? A) Fe. B) Cu. C) All the above. D) None of the above. Show Answer Correct Answer: A) Fe. 58. What happens at the anode and cathode in a galvanic cell? A) No reaction at either the anode or cathode. B) Oxidation at both the anode and cathode. C) Oxidation at the anode and reduction at the cathode. D) Reduction at the anode and oxidation at the cathode. Show Answer Correct Answer: C) Oxidation at the anode and reduction at the cathode. 59. Define electrolysis and its applications. A) Electrolysis is primarily used for cooking food. B) Electrolysis is a method for generating electricity from solar panels. C) Electrolysis is only applicable in the textile industry. D) Electrolysis is used in various applications including electroplating, purification of metals, production of chemical compounds (like chlorine and hydrogen), and in water splitting for hydrogen fuel production. Show Answer Correct Answer: D) Electrolysis is used in various applications including electroplating, purification of metals, production of chemical compounds (like chlorine and hydrogen), and in water splitting for hydrogen fuel production. 60. Nernst equation FOR (i) Mg(s) | Mg2+(0.001M) || Al3+(0.0001 M) | Al(s) A) E$_{CELL}$=E$^{0}$$_{CELL}$-0.0591/6 log[Mg2+]$^{3}$/[Al3+]$^{2}$. B) E$_{CELL}$=E$^{0}$$_{CELL}$-0.0591/6 log[Al3+]$^{2}$/[Mg2+]$^{3}$. C) E$_{CELL}$=E$^{0}$$_{CELL}$-0.0591/3 log[Mg2+] /[Al3+]. D) E$_{CELL}$=E$^{0}$$_{CELL+}$0.0591/3 log[Mg2+]$^{3}$/[Al3+]$^{2}$. Show Answer Correct Answer: A) E$_{CELL}$=E$^{0}$$_{CELL}$-0.0591/6 log[Mg2+]$^{3}$/[Al3+]$^{2}$. ← 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 5Class 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