This quiz works best with JavaScript enabled. Home > Cbse > Class 12 > Science > Chemistry Part I > Class 12 Chemistry (Part I) Chapter 3 Electrochemistry – Quiz 10 🏠 Homepage 📘 Download PDF Books 📕 Premium PDF Books Class 12 Chemistry (Part I) Chapter 3 Electrochemistry Quiz 10 (60 MCQs) Quiz Instructions Select an option to see the correct answer instantly. 1. A group of cells that are connected together A) Half cell. B) Anode. C) Battery. D) Salt bridge. Show Answer Correct Answer: C) Battery. 2. Alkaline battery is an example of A) Fuel cells. B) Primary cells. C) Electrolytic cells. D) Secondary cells. Show Answer Correct Answer: B) Primary cells. 3. In first case positive standard electrode potential is obtained due to copper is more stable than hydrogen, so Cu2+ ion get A) Oxidised. B) Dissolved. C) Reduced. D) None of the above. Show Answer Correct Answer: C) Reduced. 4. In the electrolysis of molten aluminium oxide, which of the following half equations shows the reaction at the cathode?Dalam elektrolisis leburan aluminium oksida, setengah persamaan manakah menunjukkan tindak balas di katod? A) 2O2-O2 + 4e-. B) 4OH-O2 + 2H2O + 4e-. C) Al3+ + 3e-Al. D) Al Al3+ + 3e-. Show Answer Correct Answer: C) Al3+ + 3e-Al. 5. Representation of galvanic cell in general A) Anode|electrolyte of anode (conc)|| cathode|electrolyte of cathode(conc). B) Anode |electrolyte of anode(conc)||electrolyte of cathode(conc)|cathode. C) Cathode |electrolyte of anode (conc)||anode|electrolyte of cathode (conc). D) None of the above. Show Answer Correct Answer: B) Anode |electrolyte of anode(conc)||electrolyte of cathode(conc)|cathode. 6. Which of the following are the factors that determine the type of ions to be discharged at the electrodes?I Type of electrode used.II Concentration of ions in the solution.III The molecular mass of the atom used.IV Position of ions in electrochemical series. A) I, II and III only. B) I, II and IV only. C) I, III and IV only. D) II, III and IV only. Show Answer Correct Answer: B) I, II and IV only. 7. Which metal have highest reducing power.Given the standard electrode potentials, A) Cr3+/Cr =-0.74V. B) Mg2+/Mg =-2.37 V,. C) Ag+/Ag = 0.80V,. D) Hg2+/Hg = 0.79V. E) K+/K =-2.93V,. Show Answer Correct Answer: E) K+/K =-2.93V,. 8. 1) What two metals are often used in electrochemical cells? A) Carbon and copper. B) Zinc and sulfur. C) Zinc and carbon. D) Zinc and copper. Show Answer Correct Answer: D) Zinc and copper. 9. Q5 . A salt bridge may contain A) A saturated solution of KCl and agar-agar. B) A saturated solution of KNO3 and agar-agar. C) A saturated solution of NH4NO3 and agar-agar. D) All of these. Show Answer Correct Answer: D) All of these. 10. What is the Nernst equation and its significance in electrochemistry? A) The Nernst equation is E = E$^\circ$-(RT/nF)ln(Q) and is significant for calculating cell potentials under non-standard conditions. B) The Nernst equation is irrelevant in electrochemistry. C) The Nernst equation is used to calculate reaction rates. D) The Nernst equation is E = E$^\circ$ + (RT/nF)ln(Q) for standard conditions. Show Answer Correct Answer: A) The Nernst equation is E = E$^\circ$-(RT/nF)ln(Q) and is significant for calculating cell potentials under non-standard conditions. 11. What are the products formed at the anode and the cathode during the electrolysis of molten magnesium oxide using carbon electrodes? A) Anode:Oxygen Cathode:Magnesium. B) Anode:Magnesium Cathode:Oxygen. C) Anode:Hydrogen Cathode:Oxygen. D) Anode:Oxygen Cathode:Hydrogen. Show Answer Correct Answer: A) Anode:Oxygen Cathode:Magnesium. 12. The aqueous solutions of sodium formate, anilinium chloride and potassium cyanide are respectively A) Acidic, acidic, basic. B) Basic, acidic, basic. C) Basic, neutral, basic. D) None. Show Answer Correct Answer: B) Basic, acidic, basic. 13. What concentration of Ag$^{+}$ is present in the following electrochemical cell if E =-0.683 V and E$^\circ$ (Ag$^{+}$) = +0.799 V at 25$^\circ$C?Ag | Ag$^{+}$ (? M) || H$^{+}$ (1.0 M) | H$_{2}$ (1.0 atm) | Pt A) 1.1 x 10$^{-2}$ M. B) 9.3 x 10$^{-26}$ M. C) 9.1 x 10$^{1}$ M. D) 9.1 x 10$^{-1}$ M. Show Answer Correct Answer: A) 1.1 x 10$^{-2}$ M. 14. What is a cathode? A) It is the electrode where reduction takes place. B) It is the electrode where oxidation takes place. C) It is an aqueous solution containing an electrode. D) It is the salt bridge that connects half-cells. Show Answer Correct Answer: A) It is the electrode where reduction takes place. 15. In which of the following conditions salt bridge is not required in a galvanic cell? A) When galvanic cell is used in geyser. B) When distance between oxidation half cell and reduction half cell is negligible. C) Electrolytic solutions used in both the half cells are of same concentration. D) When both the electrodes are dipped in the same electrolytic solution. Show Answer Correct Answer: D) When both the electrodes are dipped in the same electrolytic solution. 16. The unit of conductance cannot be expressed in A) Ohm/m. B) Siemen (S). C) (ohm)-1. D) Mho. Show Answer Correct Answer: C) (ohm)-1. 17. Hydrogen electrode as a reference electrode can be used as which of the following? A) Anode only. B) Salt bridge. C) Cathode only. D) Anode or Cathode. Show Answer Correct Answer: D) Anode or Cathode. 18. Which of the following is a correct representation of the Nernst equation? A) $E = E^0-\frac{nF}{RT} \ln Q$. B) $E = E^0 + \frac{nF}{RT} \ln Q$. C) $E = E^0 + \frac{RT}{nF} \ln Q$. D) $E = E^0-\frac{RT}{nF} \ln Q$. Show Answer Correct Answer: D) $E = E^0-\frac{RT}{nF} \ln Q$. 19. In an electrochemical cell, which component is responsible for allowing the flow of ions between the two half-cells? A) Salt bridge. B) Battery. C) Voltmeter. D) Electrode. Show Answer Correct Answer: A) Salt bridge. 20. During a chemistry experiment, Harper, Evelyn, and Maya are examining different electrodes. They come across a cathode. What is a cathode according to their understanding? A) It is the electrode where oxidation takes place. B) It is the salt bridge that connects half-cells. C) It is the electrode where reduction takes place. D) It is an aqueous solution containing an electrode. Show Answer Correct Answer: C) It is the electrode where reduction takes place. 21. From the following metal which is the most active one. A) Zn. B) Cu. C) Mg. D) Al. Show Answer Correct Answer: C) Mg. 22. A voltaic cell converts electrical energy to chemical energy. A) True. B) False. C) All the above. D) None of the above. Show Answer Correct Answer: B) False. 23. What is the primary function of a salt bridge in a galvanic cell? A) To allow the flow of electrons between electrodes. B) To maintain electrical neutrality by allowing the flow of ions. C) To increase the voltage of the cell. D) To prevent the mixing of different solutions. Show Answer Correct Answer: B) To maintain electrical neutrality by allowing the flow of ions. 24. A voltaic cells in which a fuel substance undergoes oxidation and from which electrical energy is continuously obtained. A) Dry cells. B) Lead storage batteries. C) Fuel cells. D) None of the above. Show Answer Correct Answer: C) Fuel cells. 25. Assuming that the redox reaction in the galvanic cell:Fe + Cu$^{2+ }$ $\rightarrow$Fe$^{2+}$ + CuWhat is the movement of electrons? A) Fe to Cu. B) Cu to Fe. C) All the above. D) None of the above. Show Answer Correct Answer: A) Fe to Cu. 26. The value which decreases with dilution is A) Conductance. B) Equivalent conductivity. C) Conductivity. D) Molar conductivity. Show Answer Correct Answer: C) Conductivity. 27. What is the importance of electrode materials in electrochemical cells? A) Electrode materials are irrelevant in determining the voltage of a cell. B) Electrode materials are essential for efficient electron transfer, affecting the performance and efficiency of electrochemical cells. C) Electrode materials are only important for aesthetic purposes. D) The choice of electrode materials has no impact on cell temperature. Show Answer Correct Answer: B) Electrode materials are essential for efficient electron transfer, affecting the performance and efficiency of electrochemical cells. 28. Which of the following reactions at an electrode is an example of oxidation? A) (text{2Cl}^-rightarrow text{Cl} 2(g) + 2text{e}^-). B) (text{Cu}^{2+} + 2text{e}^-rightarrow text{Cu}(s)). C) (text{Na}^+ + text{e}^-rightarrow text{Na}(s)). D) (text{2H} 2text{O} + 2text{e}^-rightarrow text{H} 2(g) + 2text{OH}^-). Show Answer Correct Answer: A) (text{2Cl}^-rightarrow text{Cl} 2(g) + 2text{e}^-). 29. What is the only chemical product when hydrogen and oxygen are reacted together in a fuel cell? A) Water. B) Electricity. C) Carbon dioxide. D) None of the above. Show Answer Correct Answer: A) Water. 30. Effect of acid and bases on non aqueous solvent was not explained by A) Lewis concept. B) Lowery bronsted theory. C) Arrhenius theory. D) None of the above. Show Answer Correct Answer: C) Arrhenius theory. 31. Reactions that use more energy than they produce A) Endothermic. B) Exothermic. C) Barbaric. D) Hyperbaric. Show Answer Correct Answer: A) Endothermic. 32. What is the effect of presence of electrolytes in water on corrosion of iron A) Increases. B) Decreases. C) Depends on quantity of water. D) None of the above. Show Answer Correct Answer: A) Increases. 33. A cell constructed by coupling copper and magnesium electrode has emf of 2.7 volts. if the standard reduction potential of copper electrode is +0.34 volts, that of magnesium electrode is A) 2.36v. B) +3.04. C) -3.04v. D) -2.36v. Show Answer Correct Answer: D) -2.36v. 34. The positively charged ions migrate toward the ..... A) Anode. B) Cathode. C) All the above. D) None of the above. Show Answer Correct Answer: B) Cathode. 35. Which statement is true regarding the anode in a galvanic cell? A) It is positively charged. B) It loses mass over time due to oxidation. C) It attracts anions from the solution. D) It is where the reduction reaction takes place. Show Answer Correct Answer: B) It loses mass over time due to oxidation. 36. In a Galvanic Cell, the anode species ..... A) Loses mass over the course of the rxn. B) Gains mass over the course of the rxn. C) All the above. D) None of the above. Show Answer Correct Answer: B) Gains mass over the course of the rxn. 37. How much charge is required to reduce 1 mol of Na$^{+}$ into Na? A) 2 X 96500 c. B) 96500 c. C) 3F. D) 2F. Show Answer Correct Answer: B) 96500 c. 38. What is an electrolytic cell? A) An electrolytic cell is a cell that converts electrical energy into chemical energy. B) An electrolytic cell is a cell used to convert chemical energy into electrical energy. C) An electrolytic cell is a type of battery used in cars. D) An electrolytic cell is a device that converts solar energy into electricity. Show Answer Correct Answer: A) An electrolytic cell is a cell that converts electrical energy into chemical energy. 39. When comparing voltaic cells to electrolytic cells, oxidation occurs at the A) Anode in both types of cells. B) Cathode in both types of cells. C) Anode in voltaic cells, only. D) Cathode in voltaic cells, only. Show Answer Correct Answer: A) Anode in both types of cells. 40. Galvanic cell converts A) A metal from its elemental form to combined form. B) Electrical energy into chemical energy. C) Electrolyte into individual ions. D) Chemical energy into electrical energy. Show Answer Correct Answer: D) Chemical energy into electrical energy. 41. The S.I units of molar conductivity are A) Sm 2mol-1. B) Sm2 mol-2. C) Sm-2mol. D) Sm-1 mol-1. Show Answer Correct Answer: A) Sm 2mol-1. 42. The electrolysis of molten sodium chloride produces A) Hydrochloric acid. B) Sodium liquid and chlorine gas. C) Chlorine gas and aqueous sodium hydroxide. D) Glucose. Show Answer Correct Answer: B) Sodium liquid and chlorine gas. 43. What is a balanced equation for the redox reaction represented by the twohalf-reactions below?Br$_{2}$ + 2e$^{-}$ $\rightarrow$ $\rightarrow$ A) 2Na + Br$_{2}$ $\rightarrow$. B) Na + Br$_{2 }$ $\rightarrow$. C) Na + Br$_{2}$ + e$^{-}$ $\rightarrow$. D) Na + Br$_{2}$ + 2e$^{-}$ $\rightarrow$. Show Answer Correct Answer: A) 2Na + Br$_{2}$ $\rightarrow$. 44. The nucleus of an atom is made of A) Electrons and protons. B) Electrons and neutrons. C) Protons and neutrons. D) Empty space. Show Answer Correct Answer: C) Protons and neutrons. 45. Explain the concept of corrosion and how it can be prevented using electrochemical methods. A) Anodic corrosion and cathodic corrosion. B) Chemical protection and physical protection. C) Thermal protection and mechanical protection. D) Cathodic protection and anodic protection. Show Answer Correct Answer: D) Cathodic protection and anodic protection. 46. What is the reduction potential for the half-reaction at 25$^{o}$ C:Al$^{3+}$ + 3e$^{-}$ Al, if [Al$^{3+}$] = 0.10 M and E$^{o}$ =-1.66 V? A) -1.72 V. B) -1.68 V. C) -1.66 V. D) -1.84 V. E) -1.60 V. Show Answer Correct Answer: B) -1.68 V. 47. What would be the theoretical cell potential of the previous electrochemical cell? A) -1.05V. B) 1.05V. C) -0.55V. D) 0.55V. Show Answer Correct Answer: B) 1.05V. 48. One kind of battery used in watches contains mercury(II) oxide. As current flows, the mercury(II) oxide is reduced to mercury.HgO(s) + H$_{2}$O(l) + 2e$^{-}$ $\rightarrow$ Hg(l) + 2OH$^{-}$(aq)If 2.3 x 10$^{-5}$ amperes flows continuously for 1200 days, what mass of Hg(l) is produced? (F = 96480 C/mol e$^{-}$) A) 13 g. B) 5.0 g. C) 9.9 g. D) 2.5 g. Show Answer Correct Answer: D) 2.5 g. 49. A typical half-cell consists of a piece of ..... immersed in a solution of its ions. A) Metal. B) Nonmetal. C) All the above. D) None of the above. Show Answer Correct Answer: A) Metal. 50. For the cell reaction:-2Fe$^{3+}$$_{(aq)}$ + 2I$^{-}$$_{(aq)}$ $\rightarrow$ 2Fe$^{2+}$$_{(aq)}$ + I$_{2 }$ E$^{0}$$_{cell}$ = 0.24 V at 298K. The standard Gibbs energy($\Delta$rG0) of the cell reaction is [F= 96500 C/mol] A) -46.32 kJ/mol. B) 23.16 kJ/mol. C) 46.32 kJ/mol. D) -23.16 kJ/mol. Show Answer Correct Answer: A) -46.32 kJ/mol. 51. Conductivity always ..... with a decrease in concentration A) Decreases. B) Increases. C) Remain same. D) Irregular for weak and strong. Show Answer Correct Answer: A) Decreases. 52. Which of the following are the products for the electrolysis of molten aluminium oxide? A) Oxygen gas, hydrogen gas. B) Chlorine gas, oxygen gas. C) Oxygen gas, aluminium. D) Hydrogen gas, Aluminium. Show Answer Correct Answer: C) Oxygen gas, aluminium. 53. The most powerful batteries combine strong oxidizing agents and strong reducing agents to give the largest possible ..... A) Potential difference. B) Ion mass. C) Amperage. D) Current. Show Answer Correct Answer: A) Potential difference. 54. Lithium is more easily ..... than any other metal A) Evaporated. B) Oxidized. C) Ionized. D) Reduced. Show Answer Correct Answer: B) Oxidized. 55. Which side does the electrons go on in a half reaction? A) Least Positive Side. B) Left Side. C) More Positive Side. D) Right Side. Show Answer Correct Answer: C) More Positive Side. 56. Which is the correct expression of the Gibbs free energy equation A) $\Delta G=\Delta H-T\Delta S$. B) $\Delta G=\Delta S-T\Delta H$. C) $\Delta G=\Delta H\cdot T\cdot\Delta S$. D) $\Delta G=\Delta H-\Delta TS$. Show Answer Correct Answer: A) $\Delta G=\Delta H-T\Delta S$. 57. On the electrolysis of dil. sulphuric acid using Platinum(Pt) electrode, the product obtained at anode will be A) SO$_{2}$ gas. B) O$_{2 }$ gas. C) H$_{2}$ gas. D) H$_{2}$S gas. Show Answer Correct Answer: C) H$_{2}$ gas. 58. What is the relationship between Gibbs free energy and cell potential? A) $\Delta$G =-nFE; a negative $\Delta$G indicates a positive cell potential. B) $\Delta$G =-nFE; cell potential has no relation to $\Delta$G. C) $\Delta$G = nFE; a positive $\Delta$G indicates a negative cell potential. D) $\Delta$G = 0; cell potential is always zero. Show Answer Correct Answer: A) $\Delta$G =-nFE; a negative $\Delta$G indicates a positive cell potential. 59. In the reaction:Fe + Cu$^{2+ }$ $\rightarrow$Fe$^{2+}$ + CuWhat species is reduced? A) Cu. B) Fe$^{2+}$. C) Fe. D) Cu$^{2+}$. Show Answer Correct Answer: D) Cu$^{2+}$. 60. Calculate the time to deposit 1.27 g of copper at cathode when a current of 2A was passed through the solution of CuSO4.(Molar mass of Cu = 63.5 g mol-1, 1 F = 96500 C mol-1) A) T=2930 seconds. B) T=1530 seconds. C) T=1930 seconds. D) T=1630 seconds. Show Answer Correct Answer: C) T=1930 seconds. ← 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