This quiz works best with JavaScript enabled. Home > Cbse > Class 12 > Science > Chemistry Part I > Class 12 Chemistry (Part I) Chapter 3 Electrochemistry – Quiz 13 🏠 Homepage 📘 Download PDF Books 📕 Premium PDF Books Class 12 Chemistry (Part I) Chapter 3 Electrochemistry Quiz 13 (60 MCQs) Quiz Instructions Select an option to see the correct answer instantly. 1. What is the quantity of electricity in coulombs needed to reduce 2 moles of Cu$^{2+}$ to Cu? A) 1X96500. B) 3X96500. C) 4X96500. D) 2X96500. Show Answer Correct Answer: C) 4X96500. 2. Proses pengoksidaan ialah A) Menerima elektron. B) Penerimaan oksigen. C) Bahan yang menjadi agen pengoksidaan. D) Kehilangan oksigen. Show Answer Correct Answer: B) Penerimaan oksigen. 3. Which of the following are factors affecting products in electrolysis?I Voltage of dry cellsII Position of ions in the electrochemical seriesIII Concentration of the ions in the electrolyteIV Types of electrodes used in the electrolysis A) I, II, III. B) I, III, IV. C) I, II, IV. D) II, III, IV. Show Answer Correct Answer: D) II, III, IV. 4. During an oxidation-reduction reaction there is a conservation of A) Mass only. B) Charge only. C) Mass and charge. D) Neither mass or charge. Show Answer Correct Answer: C) Mass and charge. 5. The cations in a galvanic cell moves toward the A) Cathode. B) Anode. C) All the above. D) None of the above. Show Answer Correct Answer: A) Cathode. 6. What will happen during the electrolysis of aqueous solution of CuSO$_{4 }$by using Platinum electrodes? A) Copper will dissolve at anode. B) Copper will deposit at anode. C) Copper will deposit at the cathode. D) Oxygen will be released at cathode. Show Answer Correct Answer: C) Copper will deposit at the cathode. 7. In the reaction of Cu(s) + Ni$^{2+}$(aq) $\rightarrow$ Ni (s) + Cu$^{2+}$(aq), the ..... undergoes oxidation reaction. A) Copper. B) Nickel. C) All the above. D) None of the above. Show Answer Correct Answer: A) Copper. 8. An electric current of 1.00 ampere is passed through an aqueous solution of Ni(NO$_{3}$)$_{2}$. How long will it take to plate out exactly 1.00 mol of nickel metal, assuming 100 percent current efficiency?(1 Faraday = 96, 500 coulombs) A) 193, 000 sec. B) 96, 500 sec. C) 386, 000 sec. D) 48, 200 sec. Show Answer Correct Answer: A) 193, 000 sec. 9. ..... is the reference electrode that can be used as an anode or a cathode depends on the half-cell to with it is coupled. A) Standard electrode potential. B) Standard hydrogen electrode. C) Standard cell potential. D) Electrode potential. Show Answer Correct Answer: B) Standard hydrogen electrode. 10. In any redox reaction, both oxidation and reduction must occur. A) True. B) False. C) All the above. D) None of the above. Show Answer Correct Answer: A) True. 11. A battery that remains in the inactive state and is activated immediately before use is the A) Primary battery. B) Reserve battery. C) Fuel cell. D) Secondary cell. Show Answer Correct Answer: B) Reserve battery. 12. The electrode at which ..... occurs is called the cathode. A) Oxidation. B) Reduction. C) All the above. D) None of the above. Show Answer Correct Answer: B) Reduction. 13. Nora is working on a science project where she needs to demonstrate a type of electrochemical cell that converts the chemical energy of a fuel into electrical energy. A) Salt Bridge. B) Electrolytic Cell. C) Fuel Cell. D) Anode. Show Answer Correct Answer: C) Fuel Cell. 14. Aiden is conducting an experiment with a battery. He wants to know which electrode is the site of reduction. A) Anode. B) Electrochemistry. C) Cathode. D) Oxidation. Show Answer Correct Answer: C) Cathode. 15. In a Galvanic cell, the anions from the salt bridge flow towards; A) Anode. B) Cathode. C) Both electrodes. D) None of the above. Show Answer Correct Answer: A) Anode. 16. The conductivity of an electrolyte depends on the A) Boiling point of the solvent. B) Degree of ionisation. C) Volume of the solvent. D) Molecular mass of the electrolyte. Show Answer Correct Answer: B) Degree of ionisation. 17. The standard enthalpy for an element in its reference form is defined as A) -2.0 kJ/mol. B) 0 kJ/mol. C) 2.0 kJ/mol. D) None of the above. Show Answer Correct Answer: B) 0 kJ/mol. 18. From Cr and Cu which will be oxidised? A) Cr and cu both. B) Cr. C) Cu. D) None. E) Cr. Show Answer Correct Answer: B) Cr. 19. Which of the following is a difference between a voltaic and electrolytic cell? A) Electrons flow from anode to cathode. B) Charges on anode and cathode are opposites. C) Both are used as batteries. D) Both can be used for metal plating. Show Answer Correct Answer: B) Charges on anode and cathode are opposites. 20. In metallic conductors, electrical conductivity is due to the movement of ..... A) Metals. B) Neutrons. C) Electrons. D) Protons. Show Answer Correct Answer: C) Electrons. 21. The species that is oxidized is a reductant. A) True. B) False. C) All the above. D) None of the above. Show Answer Correct Answer: A) True. 22. How can the Nernst equation be used to determine concentration? A) The Nernst equation is used to determine temperature from concentration. B) The Nernst equation calculates pressure based on volume and temperature. C) The Nernst equation provides a method to measure electrical resistance directly. D) Use the Nernst equation to calculate concentration from known cell potential and other concentrations. Show Answer Correct Answer: D) Use the Nernst equation to calculate concentration from known cell potential and other concentrations. 23. The $^{ O}$E$_{cell}$ of an electrolytic cell is A) Less than zero. B) Greater than one. C) Zero. D) Equal to one. Show Answer Correct Answer: A) Less than zero. 24. Which energy conversion shown below takes place in an electrochemical cell? A) Mechanical to electrical. B) Electrical to chemical. C) Mechanical to chemical. D) Chemical to electrical. Show Answer Correct Answer: D) Chemical to electrical. 25. Which one of the following cannot be used as anode? A) Magnesium. B) Tin. C) Zinc. D) Aluminium. Show Answer Correct Answer: B) Tin. 26. Which metal could not be used for electroplating by using an aqueous solution? A) Copper. B) Sodium. C) Silver. D) Chromium. Show Answer Correct Answer: B) Sodium. 27. The redox reaction in a galvanic cell is an example of spontaneous reaction. A) True. B) False. C) All the above. D) None of the above. Show Answer Correct Answer: A) True. 28. ..... cell converts chemical energy in to electrical energy. A) Primary. B) Secondary. C) Electrolytic. D) Electrochemical. Show Answer Correct Answer: D) Electrochemical. 29. What is the primary factor that determines the direction of electron flow in a galvanic cell? A) The size of the electrodes. B) The temperature of the cell. C) The concentration of the electrolyte. D) The difference in electrode potentials. Show Answer Correct Answer: D) The difference in electrode potentials. 30. In a voltaic cell, the half cell that receives anions from the salt bridge is A) Cathode. B) Anode. C) All the above. D) None of the above. Show Answer Correct Answer: B) Anode. 31. Which of the following is formed at the cathode during discharging process in a Ni-MH battery A) Nickel-oxy hydroxide. B) Nickel hydroxide. C) Metal hydride. D) Lithium hydroxide. Show Answer Correct Answer: B) Nickel hydroxide. 32. Based on cell notation below, give the one electrolyte can be used in cathode?Zn (s) /Zn$^{2+ }$(aq, 1M) // H$^{+ }$(aq, 1M) / H$_{2 }$(g, 1 atm)/graphite (s) A) ZnCl$_{2}$(aq). B) ZnSO$_{4}$(aq). C) HCl(aq). D) H$_{2}$(aq). Show Answer Correct Answer: C) HCl(aq). 33. Explain the significance of standard hydrogen electrode. A) The significance of the standard hydrogen electrode lies in its role as a reference point for measuring electrode potentials. B) The standard hydrogen electrode is primarily used in organic chemistry experiments. C) It is a tool for measuring temperature in chemical reactions. D) The standard hydrogen electrode is used for electrolysis in batteries. Show Answer Correct Answer: A) The significance of the standard hydrogen electrode lies in its role as a reference point for measuring electrode potentials. 34. Do cathodes gain mass? A) Yes. B) No. C) All the above. D) None of the above. Show Answer Correct Answer: A) Yes. 35. Debye Huckel-Onsager equation is found to hold goodat A) Low concentrations. B) Moderate concentrations. C) Does not hold good at change of concentrations. D) High Concentrations. Show Answer Correct Answer: A) Low concentrations. 36. With decrease in concentration, molar conductivity A) Decreases. B) Increases. C) Remains constant. D) None. Show Answer Correct Answer: B) Increases. 37. What is the primary purpose of a salt bridge in an electrochemical cell? A) To act as a catalyst. B) To maintain electrical neutrality. C) To increase the cell voltage. D) To generate electricity. Show Answer Correct Answer: B) To maintain electrical neutrality. 38. Which of the following assertions about the main cell is correct? A) An example of a primary cell is a mercury cell. B) An example of a primary cell is a nickel-cadmium storage cell. C) It can be recharged. D) The electrode reactions can be reversed. Show Answer Correct Answer: A) An example of a primary cell is a mercury cell. 39. In a Galvanic Cell, the cathode is ..... A) Positive. B) Negative. C) All the above. D) None of the above. Show Answer Correct Answer: A) Positive. 40. Which of the following is a disadvantage of using hydrogen as a fuel? A) There are currently very few hydrogen filling stations in the UK. B) It directly contributes to global warming. C) Hydrogen is radioactive. D) None of the above. Show Answer Correct Answer: A) There are currently very few hydrogen filling stations in the UK. 41. Highest magnetic moment is shown by the ion-: A) Co$^{+3}$. B) Cr$^{+3}$. C) Fe$^{+3}$. D) V$^{+2}$. Show Answer Correct Answer: C) Fe$^{+3}$. 42. Define equivalent conductivity. A) The conducting power of all ions furnished by one gram equivalent of electrolyte in a definite volume of solution. B) The conductance of all ions furnished by one gram equivalent of electrolyte in a definite volume of solution. C) The resistance of all ions furnished by one gram equivalent of electrolyte in a definite volume of solution. D) None of the above. Show Answer Correct Answer: A) The conducting power of all ions furnished by one gram equivalent of electrolyte in a definite volume of solution. 43. Which of the following is the SI unit of conductivity. A) S m$^{-1}$. B) S m$^{2}$ mol$^{-2}$. C) S m$^{2}$ mol. D) S m$^{2}$ mol$^{-1}$. Show Answer Correct Answer: A) S m$^{-1}$. 44. The unit of specific conductance (k) is A) Ohm cm-1. B) Ohm-1 cm. C) Ohm-1 cm-1. D) Ohm cm. Show Answer Correct Answer: C) Ohm-1 cm-1. 45. The electrolyte for both half-cells in a lead storage battery is ..... A) Sodium hydroxide. B) Hydrochloric acid. C) Sulfuric acid. D) None of the above. Show Answer Correct Answer: C) Sulfuric acid. 46. How can you calculate the cell potential using the Nernst equation? A) E = E$^\circ$ + (nF/RT) * log(Q). B) E = E$^\circ$ + (RT/nF) * ln(Q). C) E = E$^\circ$-(RT/nF) * ln(Q). D) E = E$^\circ$-(nF/RT) * ln(Q). Show Answer Correct Answer: C) E = E$^\circ$-(RT/nF) * ln(Q). 47. In a galvanic cell, it is an electrode where the oxidation happens? A) Cathode Electrode. B) Anode Electrode. C) All the above. D) None of the above. Show Answer Correct Answer: B) Anode Electrode. 48. Which metal is the negative electrode? A) Zinc. B) Copper. C) All the above. D) None of the above. Show Answer Correct Answer: A) Zinc. 49. Aqueous solution of which of the following compounds is the best conductor of electric current. A) HCl. B) Acetic acid. C) Ammonia. D) Fructose. Show Answer Correct Answer: A) HCl. 50. Which of the following will NOT affect the selective discharge of ions? A) Type of electrolyte. B) Concentration of ions in electrolysis. C) Position of ions in the electrochemical series. D) Type of electrodes. Show Answer Correct Answer: A) Type of electrolyte. 51. What is the function of porous pot in Daniel Cell ..... ? A) To complete the circuit. B) Enable the movement of ion. C) Dont mix the solution. D) None of the above. Show Answer Correct Answer: B) Enable the movement of ion. 52. In voltaic cells, the salt bridge ..... A) Is not necessary in order for the cell to work. B) Acts as a mechanism to allow mechanical mixing of the solutions. C) Allows charge balance to be maintained in the cell. D) Drives free electrons from one half-cell to the other. Show Answer Correct Answer: C) Allows charge balance to be maintained in the cell. 53. Harper and Anika are conducting a chemistry experiment. They are observing a reaction where one reactant loses electrons and the other gains them. What type of reaction are they observing? A) A reaction where both reactants get reduced. B) A reaction where both reactants get oxidized. C) A reaction that involves a transfer of electrons between reactants. D) A reaction that involves the combustion of at least one reactant. Show Answer Correct Answer: C) A reaction that involves a transfer of electrons between reactants. 54. In electrolysis, what is the role of the anode? A) To receive electrons from the electrolyte. B) To convert electrical energy into chemical energy. C) To supply electrons to the electrolyte. D) To convert chemical energy into electrical energy. Show Answer Correct Answer: A) To receive electrons from the electrolyte. 55. The resistance of a solution 'A' is 40 ohm and that of solution 'B' is 70 ohm, both solutions being taken in the same conductivity cell. If equal volumes of solutions 'A' and 'B' are mixed, what will be the resistance of the mixture using the same cell? (Assume that there is no increase in the degree of dissociation of 'A' and 'B' on mixing) A) 50 ohm. B) 50.9 ohm. C) 101.8 ohm. D) 110 ohm. Show Answer Correct Answer: B) 50.9 ohm. 56. Which of the following is true about the Danielle cell? A) The cathode is negatively charged. B) The electron flows from anode to cathode outside the cell. C) The e.m.f is 1.5V. D) Electricity flows from the zinc electrode to the copper electrode outside the cell. Show Answer Correct Answer: B) The electron flows from anode to cathode outside the cell. 57. How many Faraday's are required to oxidize 1 mole of H$_{2}$O to O$_{2}$. A) 3. B) 1. C) 4. D) 2. Show Answer Correct Answer: D) 2. 58. Which of the following statement regarding Concentration cell is incorrect A) Electrode which is in contact with the solution of lower concentration acts as cathode. B) Electrode which is in contact with the solution of lower concentration acts as anode. C) Electrode which is in contact with the solution of higher concentration undergoes reductin. D) Electrode which is in contact with the solution of lower concentration undergoes oxidation. Show Answer Correct Answer: A) Electrode which is in contact with the solution of lower concentration acts as cathode. 59. An electrolytic cell differs from a voltaic cell because an electrolytic cell A) Generates its own energy from a spontaneous physical reaction. B) Requires an outside energy source for a nonspontaneous chemical reaction to occur. C) Generates its own energy from a nonspontaneous physical reaction. D) Requires an outside energy source for a spontaneous chemical reaction to occur. Show Answer Correct Answer: B) Requires an outside energy source for a nonspontaneous chemical reaction to occur. 60. The charge required for the reduction of 1 mol of MnO$_{4}$$^{-}$ to MnO$_{2}$ is A) 6 F. B) 1 F. C) 3 F. D) 4 F. Show Answer Correct Answer: C) 3 F. ← 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