This quiz works best with JavaScript enabled. Home > Cbse > Class 12 > Science > Chemistry Part I > Class 12 Chemistry (Part I) Chapter 3 Electrochemistry – Quiz 14 🏠 Homepage 📘 Download PDF Books 📕 Premium PDF Books Class 12 Chemistry (Part I) Chapter 3 Electrochemistry Quiz 14 (60 MCQs) Quiz Instructions Select an option to see the correct answer instantly. 1. The quantity of electricity required in Faraday for oxidation of one mol of ferrous oxide to ferric oxide A) 1. B) 2. C) 4. D) None of the above. Show Answer Correct Answer: A) 1. 2. How is cell potential calculated? A) Ecell = Ecathode x Eanode. B) Ecell = Ecathode / Eanode. C) Ecell = Ecathode + Eanode. D) Ecell = Ecathode-Eanode. Show Answer Correct Answer: D) Ecell = Ecathode-Eanode. 3. You have two copper electrodes and a solution of CuSO4. What will happen to the negative pole of the Copper electrodes? A) It will turn black. B) It will shrink. C) A gas will bubble off. D) It will get bigger. Show Answer Correct Answer: D) It will get bigger. 4. What is the significance of the standard hydrogen electrode in electrochemistry? A) It provides a known and consistent reduction potential of 0 V at all conditions. B) It is only applicable in specific temperature ranges. C) It is used as a reference electrode in all electrochemical cells. D) It measures the potential of all electrodes in a solution. Show Answer Correct Answer: A) It provides a known and consistent reduction potential of 0 V at all conditions. 5. To eliminate liquid junction potential is by placing the salt bridge in an electrochemical cell? A) True. B) False. C) All the above. D) None of the above. Show Answer Correct Answer: A) True. 6. State one functions of salt bridge A) To maintain the movement of electron. B) To allowing electron to flow and complete the circuit. C) To separate two electrolyte. D) To allowing movement of ion to complete the circuit. Show Answer Correct Answer: D) To allowing movement of ion to complete the circuit. 7. Which of the following is the correct half cell equation at anode for the spontaneous redox reaction.Pb$^{2+}$ + Fe$^{2+}$ $\rightarrow$ Fe$^{3+}$ + Pb A) Pb$^{2+ }$+ 2e$^{-}$$\rightarrow$ Pb. B) Pb $\rightarrow$ Pb$^{2+ }$+ 2e$^{-}$. C) Fe$^{3+ }$+ e$^{-}$$\rightarrow$ Fe$^{2+}$. D) Fe$^{2+}$ $^{ }$$\rightarrow$ Fe$^{3+ }$+ e$^{-}$. Show Answer Correct Answer: B) Pb $\rightarrow$ Pb$^{2+ }$+ 2e$^{-}$. 8. Difference between equivalent conductance and molar conductance is ..... A) Concentration. B) Pressure. C) Temperature. D) Volume. Show Answer Correct Answer: A) Concentration. 9. Amount of Ca metal deposit at electrode during electrolysis of molten CaCl2 by 15A current for 20 minute is A) 3g approx. B) 5g approx. C) 4g approx. D) 6g approx. Show Answer Correct Answer: A) 3g approx. 10. Which of the following is true using the following electrochemical reaction:Mn/Mn(NO3)2 // PBSO4/Pb A) Pb is oxidized. B) A strip of Pb is put into solution of Mn(NO3)2. C) Electrons are lost at the Mn electrode. D) Mn is reduced. Show Answer Correct Answer: C) Electrons are lost at the Mn electrode. 11. Inert electrolyte in salt bridge reacts with solution of half cells A) Insufficient data. B) False. C) Cant explain. D) True. Show Answer Correct Answer: B) False. 12. An electrochemical cell that is used to convert chemical energy into electrical energy A) Voltaic cell. B) Electrolysis. C) Electrode. D) Anode. Show Answer Correct Answer: A) Voltaic cell. 13. Three factors affecting the selection of species to be discharged at electrodes except ..... A) Standard reduction potential of the species. B) Concentration of the species. C) Nature of electrodes (active or inert). D) Mass of the species. Show Answer Correct Answer: D) Mass of the species. 14. The driving force of such a voltaic cell is the spontaneous ..... between zinc metal and copper ions in solution. A) Combustion reaction. B) Redox reaction. C) Decomposition reaction. D) None of the above. Show Answer Correct Answer: B) Redox reaction. 15. Samuel observed a metal object rusting over time and realized it was due to the loss of electrons. A) Electrochemistry. B) Oxidation. C) Anode. D) Electrolysis. Show Answer Correct Answer: B) Oxidation. 16. A conductivity cell containing electrodes made up of A) Copper. B) Platinum. C) Iron. D) Silver. Show Answer Correct Answer: B) Platinum. 17. The ..... force (EMF) is the maximum electrical potential difference between two electrodes or half-cells of a galvanic or voltaic cell. A) ELECTROMOTIVE. B) ELECTROMAGNETIC. C) ELECTROMETALLIC. D) ELECTROMECHANIC. Show Answer Correct Answer: A) ELECTROMOTIVE. 18. When solid iron is oxidized to Fe$^{2+}$$_{(aq)}$ by CuNO$_{3}$ at 25$^\circ$C, the standard cell potential is 0.927 V. What is $\Delta$G$^\circ$? A) -179 kJ. B) -89 kJ. C) +89 kJ. D) +179 kJ. Show Answer Correct Answer: A) -179 kJ. 19. When a piece of metal M is placed in an iron(II) sulphate solution, a grey deposit is formed. Metal M may beApabila sekeping logam M diletakkan di dalam larutan ferum(II) sulfat, suatu enapan kelabu terbentuk. Logam M mungkin ialah A) LeadPlumbum. B) SilverArgentum. C) CopperKuprum. D) AluminiumAluminium. Show Answer Correct Answer: B) SilverArgentum. 20. The emf of the cell:Ni / Ni$^{2+}$ (1.0 M) // Au$^{3+}$ (1.0 M) / Au (E$^\circ$ =-0.25 V for Ni$^{2+}$/Ni; E$^\circ$ = 1.5 V for Au$^{3+}$/Au) is A) 1.75 V. B) 1.25 V. C) -1.25 V. D) 2.0 V. Show Answer Correct Answer: A) 1.75 V. 21. Reactions in galvanic/voltaic cells are A) Spontaneous, redox reactions. B) Spontaneous, non-redox reactions. C) Non-spontaneous, redox reactions. D) Non-spontaneous, non-redox reactions. Show Answer Correct Answer: A) Spontaneous, redox reactions. 22. During the operation of a galvanic cell, the mass of the cathode will ..... A) Increase. B) Remain unchanged. C) Decrease. D) First decrease, then increase. Show Answer Correct Answer: A) Increase. 23. What is the charge of a single element in a half reaction? A) 0. B) +2. C) +3. D) +1. Show Answer Correct Answer: A) 0. 24. Table J tells ..... A) Which compound is molecular. B) Whether a charge of an atom is positive or negative. C) Whether a compound is Metallic or Ionic. D) How reactive an element is and if it's spontaneous. Show Answer Correct Answer: D) How reactive an element is and if it's spontaneous. 25. Two Faraday of electricity is passed through a solution of CuSO$_{4}$. The mass of copper deposited at the cathode is:(at. mass of Cu = 63.5 amu) A) 0 g. B) 63.5 g. C) 127 g. D) 2 g. Show Answer Correct Answer: B) 63.5 g. 26. Electrochemistry deals with the interrelationship between ..... energy and chemical energy. A) Potential. B) Mechanical. C) Kinetic. D) Electrical. Show Answer Correct Answer: D) Electrical. 27. Gibbs free-energy change is the ( ) amount of energy that can be ( ) another process to do useful work A) Minimum duplicated by. B) Spontaneous, coupled to. C) Maximum, coupled to. D) Maximum, duplicated by. Show Answer Correct Answer: C) Maximum, coupled to. 28. In the hydrogen-oxygen fuel cell, ..... flows into the cathode compartment. A) Carbon dioxide. B) Oxygen. C) Hydrogen. D) None of the above. Show Answer Correct Answer: B) Oxygen. 29. What kind of notation is best used for voltaic cells? A) Shorthand notation. B) Longhand notation. C) Salt bridge notation. D) Drawings. Show Answer Correct Answer: A) Shorthand notation. 30. Explain the role of electrodes in electrochemical cells. A) Electrodes facilitate oxidation and reduction reactions, generating electric current in electrochemical cells. B) Electrodes prevent chemical reactions from occurring. C) Electrodes are used to store energy in batteries. D) Electrodes only serve as connectors in circuits. Show Answer Correct Answer: A) Electrodes facilitate oxidation and reduction reactions, generating electric current in electrochemical cells. 31. Electrolysis will NOT work when the compound is in a solid state because ..... A) The ions are not present. B) The ions are free to move. C) The ions are arranged in rows. D) The ions are not free to move. Show Answer Correct Answer: D) The ions are not free to move. 32. What is the role of the reduction potential in electrolytic cells? A) It increases the concentration of the electrolyte solution. B) It decreases the cell potential. C) It is irrelevant to the operation of electrolytic cells. D) It determines the amount of energy required to drive the non-spontaneous reaction. Show Answer Correct Answer: D) It determines the amount of energy required to drive the non-spontaneous reaction. 33. A voltaic cell uses tin and aluminum for the electrodes. When the battery is operating the electrons will flow from A) Half cell 1 to half cell 2 through the salt bridge. B) Sn to Al. C) The battery will not function spontaneously. D) Al to Sn. Show Answer Correct Answer: D) Al to Sn. 34. If the E$_{cell}$ is <0, the reaction is A) Spontaneous. B) Non-spontaneous. C) All the above. D) None of the above. Show Answer Correct Answer: B) Non-spontaneous. 35. Cu$^{2+}$(aq) + 2e$^{-}$$\rightarrow$Cu(s) E$^\circ$ = 0.34 VCr$^{3+}$(aq) + e$^{-}$$\rightarrow$Cr$^{2+}$(aq) E$^\circ$ =-0.41 V A) Cu(s) + 2Cr$^{3+}$(aq) $\rightarrow$ Cu$^{2+}$(aq) + 2Cr$^{2+}$(aq). B) Cu(s) + Cr$^{3+}$(aq) $\rightarrow$ Cu$^{2+}$(aq) + Cr$^{2+}$(aq). C) Cu$^{2+}$(aq) + Cr$^{3+}$(aq) $\rightarrow$ Cu(s) + Cr$^{2+}$(aq). D) Cu$^{2+}$(aq) + 2Cr$^{2+}$(aq) $\rightarrow$ Cu(s) + 2Cr$^{3+}$(aq). Show Answer Correct Answer: D) Cu$^{2+}$(aq) + 2Cr$^{2+}$(aq) $\rightarrow$ Cu(s) + 2Cr$^{3+}$(aq). 36. Jenny wants to make her ring more beautiful and prevent corrosion. What is the best way to achieve this? A) Polished the ring with water. B) Plate the ring with gold. C) Wash the ring with soap. D) Dip the ring in oil. Show Answer Correct Answer: B) Plate the ring with gold. 37. What would be the cell potential of this electrochemical cell?Ag$^{+}$/Ag = 0.80VNi$^{2+}$/Ni =-0.25V A) 0.55V. B) 1.05V. C) -1.05V. D) -0.55V. Show Answer Correct Answer: B) 1.05V. 38. An iron nail is put into a solution of copper nitrate, copper has a more positive reduction potential than iron, what will happen? A) Bubbles of oxygen gas will form on iron nail. B) No reaction occurs. C) Iron will be reduced. D) The iron nail will become copper plated. Show Answer Correct Answer: D) The iron nail will become copper plated. 39. What is an anode? A) It is an aqueous solution containing an electrode. B) It is the salt bridge that connects half-cells. C) It is the electrode where reduction takes place. D) It is the electrode where oxidation takes place. Show Answer Correct Answer: D) It is the electrode where oxidation takes place. 40. The electrolyte has to contain A) Ions of the plating metal. B) Any type of metal. C) No metal ions. D) The metal to be plated. Show Answer Correct Answer: A) Ions of the plating metal. 41. The charge carry by 1 mole electron is A) 9650 C. B) 96.5 C. C) 96500 C. D) 965 C. Show Answer Correct Answer: C) 96500 C. 42. Graphite is used as an electrode because it A) Does not burn. B) Is a reducing agent. C) Is a metal. D) Has mobile electrons. Show Answer Correct Answer: D) Has mobile electrons. 43. Rusting can be prevented by A) Alloying. B) Tinning. C) Galvanizing. D) All of above. Show Answer Correct Answer: D) All of above. 44. The electrolysis of water produces A) Acids and bases. B) Hydrogen gas only. C) Hydrogen gas and oxygen gas. D) Oxygen gas only. Show Answer Correct Answer: C) Hydrogen gas and oxygen gas. 45. Reference electrode that is universally used whose reduction potential value is zero is A) SHE. B) Calomel electrode. C) Chlorine electrode. D) Standard zinc electrode. Show Answer Correct Answer: A) SHE. 46. Which metal reacts spontaneously with NiCl2(aq)? A) Zn(s). B) Cu(s). C) Au(s). D) Sn(s). Show Answer Correct Answer: A) Zn(s). 47. In an electrochemical cell, what does the Nernst equation predict when the concentrations of reactants and products are equal? A) The cell potential is zero. B) The cell potential is at its maximum. C) The cell potential equals the standard cell potential. D) The cell potential is negative. Show Answer Correct Answer: C) The cell potential equals the standard cell potential. 48. The number of Faradays(F) required to produced 20 g of calcium from molten CaCl$_{2}$ is (Atomic mass of Ca = 40 g/mol) A) 4. B) 1. C) 2. D) 3. Show Answer Correct Answer: B) 1. 49. For spontaneity of a cell, which is correct? A) G =-ve E O = 0. B) G = +ve EO = 0. C) G =-ve EO = + ve. D) G=0 Eo = 0. Show Answer Correct Answer: C) G =-ve EO = + ve. 50. In electroplating, which of the following is true about the object to be plated? A) It is used as the cathode. B) It is connected to the positive terminal of the power supply. C) It is used as the anode. D) It is immersed in a non-conductive solution. Show Answer Correct Answer: A) It is used as the cathode. 51. In an electrolytic cell, which electrode is connected to the positive terminal of the battery? A) Cathode. B) Positive electrode. C) Anode. D) Negative electrode. Show Answer Correct Answer: C) Anode. 52. Mason and David are setting up an electrochemical cell for their science project. They need a junction that connects the anodic and cathodic compartments (half-cells) in their setup. A) Electrochemistry. B) Anode. C) Electrolysis. D) Salt Bridge. Show Answer Correct Answer: D) Salt Bridge. 53. Electro-clumping is an innovative technique for treating ..... A) Sick animals. B) Rubbish. C) Wastewater. D) Sick plants. Show Answer Correct Answer: C) Wastewater. 54. A reactions that produces more energy than it takes in A) Barbaric. B) Endothermic. C) Exothermic. D) Hyperbaric. Show Answer Correct Answer: C) Exothermic. 55. How is voltaic cell electricity produced? A) It injects itself. B) It is pumped into the cell. C) An injected chemical reaction. D) A chemical reaction. Show Answer Correct Answer: D) A chemical reaction. 56. What is the effect of increasing the concentration of reactants in an electrochemical cell? A) It increases the cell potential. B) It has no effect on the cell potential. C) It reverses the direction of the reaction. D) It decreases the cell potential. Show Answer Correct Answer: A) It increases the cell potential. 57. Without losing its concentration ZnCl2 solution cannot be kept in contact with A) Ag. B) Al. C) Pb. D) Au. Show Answer Correct Answer: B) Al. 58. The equilibrium constants of two redox reactions X and Y are 1.5 x10$^{15}$ and 5.5 x 10$^{16}$ . Reaction X is more spontaneous than Y. A) FALSE. B) TRUE. C) All the above. D) None of the above. Show Answer Correct Answer: A) FALSE. 59. In the following reactionSn$^{2+}$ + 2Fe$^{3+}$ $\rightarrow$ Sn$^{4+ }$+ 2Fe$^{2+}$the oxidizing agent is ..... A) Fe$^{3+}$. B) Sn$^{2+}$. C) Sn$^{4+}$. D) Fe$^{2+}$. Show Answer Correct Answer: A) Fe$^{3+}$. 60. A higher reduction potential in a galvanic cell indicates that a substance is more likely to: A) Act as an electrolyte. B) Undergo oxidation. C) Undergo reduction. D) Remain inert. Show Answer Correct Answer: C) Undergo reduction. ← 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 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 8 🏠 Back to Homepage 📘 Download PDF Books 📕 Premium PDF Books