This quiz works best with JavaScript enabled. Home > Cbse > Class 12 > Science > Chemistry Part I > Class 12 Chemistry (Part I) Chapter 3 Electrochemistry – Quiz 9 🏠 Homepage 📘 Download PDF Books 📕 Premium PDF Books Class 12 Chemistry (Part I) Chapter 3 Electrochemistry Quiz 9 (60 MCQs) Quiz Instructions Select an option to see the correct answer instantly. 1. In the reaction:Fe + Cu$^{2+ }$ $\rightarrow$Fe$^{2+}$ + CuHow many electrons are lost? A) 6. B) 2. C) 0. D) 4. Show Answer Correct Answer: B) 2. 2. Depression of freezing point is used in A) Debye Falkenhagen effect. B) Osmotic coefficient. C) Wien effect. D) Debye Huckel Onsager equation. Show Answer Correct Answer: B) Osmotic coefficient. 3. Describe the role of ions in electrochemical cells. A) Ions are used to store energy in electrochemical cells. B) Ions do not affect the flow of electricity in electrochemical cells. C) Ions facilitate electric current flow by moving between the anode and cathode in electrochemical cells. D) Ions are only present at the cathode in electrochemical cells. Show Answer Correct Answer: C) Ions facilitate electric current flow by moving between the anode and cathode in electrochemical cells. 4. What reaction occurs at the anode?Ag$^{+}$/Ag = 0.80VNi$^{2+}$/Ni =-0.25V A) Ni$^{2+}$ + 2e$^{-}$ $\rightarrow$ Ni. B) Ag $\rightarrow$ Ag$^{+}$ + e$^{-}$. C) Ag$^{+}$ + e$^{-}$ $\rightarrow$Ag. D) Ni $\rightarrow$ Ni$^{2+}$ + 2e$^{-}$. Show Answer Correct Answer: D) Ni $\rightarrow$ Ni$^{2+}$ + 2e$^{-}$. 5. Which of the following statements is not correct about an inert electrode in a cell? A) It provides surface for redox reaction. B) It provides surface for conduction of electrons. C) It provides surface either for oxidation or for reduction reaction. D) It does not participate in the cell reaction. Show Answer Correct Answer: A) It provides surface for redox reaction. 6. What occurs to the mass of copper electrode in the following reaction?Zn/Zn$^{2+}$ // Cu$^{2+}$/Cu A) Increases. B) Decreases. C) Remains the same. D) None of the above. Show Answer Correct Answer: A) Increases. 7. Which metal is the negative electrode?Zn/Zn$^{2+}$ // Cu$^{2+}$/Cu A) Zinc. B) Copper. C) All the above. D) None of the above. Show Answer Correct Answer: A) Zinc. 8. The energy stored in chemical compounds is called A) Chemical energy. B) Thermal energy. C) Potential energy. D) None of the above. Show Answer Correct Answer: A) Chemical energy. 9. What does the double line mean?Zn/Zn+2 // Cu+2/Cu A) Substance in contact. B) Cathode. C) Anode. D) Salt bridge. Show Answer Correct Answer: D) Salt bridge. 10. Which one is dead cell A) Lechlenche cell. B) Mercury cell. C) Primary batteries. D) All of these. Show Answer Correct Answer: D) All of these. 11. Electronic conductors deals with A) Liquids. B) Gases. C) Solids. D) All of the above. Show Answer Correct Answer: C) Solids. 12. It is the positive or oxidizing electrode that acquires electrons from the external circuit and is reduced during the electrochemical reaction. A) Cathode. B) Anode. C) Diode. D) Electrode. Show Answer Correct Answer: A) Cathode. 13. Discuss the importance of electrochemical cells in energy storage. A) Electrochemical cells have no importance in energy storage. B) Electrochemical cells are not essential for energy storage. C) Electrochemical cells are important for converting chemical energy into electrical energy and vice versa, making them essential for energy storage in batteries and fuel cells. D) Electrochemical cells are only used for storing mechanical energy. Show Answer Correct Answer: C) Electrochemical cells are important for converting chemical energy into electrical energy and vice versa, making them essential for energy storage in batteries and fuel cells. 14. Which device requires electrical energy to produce a chemical change? A) Voltmeter. B) Salt bridge. C) Voltaic cell. D) Electrolytic cell. Show Answer Correct Answer: D) Electrolytic cell. 15. What does the charge of an anode depend on? A) If it oxidizes. B) Whether it is electrolytic or voltaic. C) If it contains a cathode. D) The charge of the anodes. Show Answer Correct Answer: B) Whether it is electrolytic or voltaic. 16. In the Nernst equation, what does the term $RT/nF$ A) The change in free energy. B) The temperature dependence of the cell potential. C) The standard cell potential. D) The equilibrium constant. Show Answer Correct Answer: B) The temperature dependence of the cell potential. 17. What is a galvanic cell and how does it work? A) A type of cell used for storing sound energy. B) A type of cell used for storing heat energy. C) An electrochemical cell that converts chemical energy into electrical energy by using spontaneous redox reactions. D) A device that converts mechanical energy into electrical energy. Show Answer Correct Answer: C) An electrochemical cell that converts chemical energy into electrical energy by using spontaneous redox reactions. 18. The cathode in a Nickel metal hydride battery consists of A) Nickel oxy hydroxide. B) Hydrides of metals. C) Aqueous solution of KOH. D) None of these. Show Answer Correct Answer: A) Nickel oxy hydroxide. 19. What is an oxidation number? A) Charge of Atom or electrons gained/lost. B) The number of protons that an element has. C) A reaction between oxidation of an atom. D) The number of element ions. Show Answer Correct Answer: A) Charge of Atom or electrons gained/lost. 20. An example of a cation is ..... A) $Cl^-$. B) $Cl_2$. C) Na. D) $Na^+$. Show Answer Correct Answer: D) $Na^+$. 21. If the cell potential is negative, the reaction is? A) A success. B) Spontaneous. C) Not spontaneous. D) None of the above. Show Answer Correct Answer: C) Not spontaneous. 22. The product of conductivity of an electrolyte and the volume containing one gram mole of the electrolyte is known as A) Molar conductance. B) Specific conductance. C) Equivalent conductance. D) Conductance. Show Answer Correct Answer: A) Molar conductance. 23. A current was passed for 5 hours through two electrolytic cells connected in series. The first cell contains AuCl$_{3}$ and second cell CuSO$_{4}$ solution. If 9.85 g of gold was deposited in the first cell, what amount of copper gets deposited in the second cell?Given:Atomic mass of Au = 197 amu and Cu = 63.5 amu. (Comptt. All India 2013) A) 3.2g. B) 3.7g. C) 4.8g. D) 5.5 g. Show Answer Correct Answer: C) 4.8g. 24. Calculate the standard cell potential.Ni + 2Fe+3 $\rightarrow$ Ni+2 + Fe+2 A) -0.19 V. B) -1.02 V. C) 1.02 V. D) -0.286 V. Show Answer Correct Answer: C) 1.02 V. 25. Determine the $\Delta$G, use F= 96458 J/V mol e$^{-}$:+0.434 V, n = 2 A) 83748.98 J/mol. B) -83748.98 J/mol. C) -83.760 kJ/mol. D) 84 kJ/mol. Show Answer Correct Answer: B) -83748.98 J/mol. 26. Consider the half-cell reaction(s) Cu$^{2+}$+e$\rightarrow$Cu+;Eo=0.15V Cu$^{2+}$+2e$\rightarrow$Cu;Eo=0.33V Eo for the half-cell reaction:Cu$^{+}$+e$\rightarrow$Cu will be: A) .18 V. B) .31 V. C) .48 V. D) .51 V. Show Answer Correct Answer: D) .51 V. 27. During a chemistry experiment, William and Ethan were discussing the role of a reducing agent. What is a reducing agent? A) It is the species that gets reduced gains electrons. B) It is the species that gets oxidized loses electrons. C) It is the species that creates electrons. D) It is the species that destroys electrons. Show Answer Correct Answer: B) It is the species that gets oxidized loses electrons. 28. When a voltaic cell operates, ions move through the A) Anode. B) Salt bridge. C) External circuit. D) Cathode. Show Answer Correct Answer: B) Salt bridge. 29. What are the cations present in zinc sulphate solution? A) OH$^{-}$, SO$_{4}$$^{2-}$. B) Zn$^{2+}$, SO$_{4}$$^{2}$. C) Zn$^{2+ }$, H$^{+}$. D) Zn$^{2+}$. Show Answer Correct Answer: C) Zn$^{2+ }$, H$^{+}$. 30. Debye Huckel-Onsager equation curve obtained for a weakelectrolyte shows that there is a very largeincrease in conductance with dilution especially near A) Zero dilution. B) Small dilution. C) Large dilution. D) Infinite dilution. Show Answer Correct Answer: D) Infinite dilution. 31. In the reaction:Fe + Cu$^{2+ }$ $\rightarrow$Fe$^{2+}$ + CuWhich half-reaction can be found in the cathode? A) Fe$\rightarrow$ Fe$^{2+ }$+ 2e$^{-}$. B) Fe + 2e$\rightarrow$ Fe$^{2+}$. C) Cu +2e $\rightarrow$ Cu$^{2+}$. D) Cu$^{2+}$ + 2e$^{-}$$\rightarrow$ Cu. Show Answer Correct Answer: D) Cu$^{2+}$ + 2e$^{-}$$\rightarrow$ Cu. 32. ..... is a compound that are able to conduct electric current whether in molten or aqueous solution and undergoes chemical changes. A) Electrolyte. B) Electrodes. C) Non-electrolyte. D) Electrolysis. Show Answer Correct Answer: A) Electrolyte. 33. The e.m.f. of the cell Pt(s) |H$_{2}$(g)|H$^{+}$(aq)||Ag$^{+}$(aq)|Ag(s) would be increased by A) Decreasing the pressure of H$_{2}$(g). B) Increasing the surface area of the Pt electrode. C) Increasing the concentration of Ag$^{+}$(aq). D) Increasing the concentration of H$^{+}$(aq). Show Answer Correct Answer: C) Increasing the concentration of Ag$^{+}$(aq). 34. Which of the following metals is MOST COMMONLY USED as an electrical conductor due to its price and abundance. A) ZINC. B) PLATINUM. C) SILVER. D) COPPER. Show Answer Correct Answer: D) COPPER. 35. The charge of cathode in a galvanic cell A) +. B) -. C) 0. D) None of the above. Show Answer Correct Answer: A) +. 36. The unit of conductivity is A) Ohm-1cm-1. B) Ohm-1. C) Ohm-1cm2eq-1. D) Ohm-1cm2. Show Answer Correct Answer: A) Ohm-1cm-1. 37. In a voltaic cell the purpose of the salt bridge is to A) All electrons to move between the two half cells. B) Block the flow of electrons. C) Allow the flow of ions between the two half cells. D) Block th eflow of ionbs between the two half cells. Show Answer Correct Answer: C) Allow the flow of ions between the two half cells. 38. Explain how batteries utilize electrochemical principles. A) Batteries utilize electrochemical principles by converting chemical energy into electrical energy through oxidation and reduction reactions at the electrodes. B) Batteries operate solely on thermal energy without chemical reactions. C) Batteries store energy by trapping light in solar cells. D) Batteries generate energy through mechanical movement of parts. Show Answer Correct Answer: A) Batteries utilize electrochemical principles by converting chemical energy into electrical energy through oxidation and reduction reactions at the electrodes. 39. For the cell reaction Z n + Cu$^{2+}$ ..... > Zn$^{2+}$ +Cucell representation is A) Cu$^{2+}$/Zn/ // Zn$^{2+}$/Cu. B) Cu$^{2+}$/Cu //Zn/Zn$^{2+}$. C) Zn/Zn$^{2+}$ // Cu$^{2+}$/Cu. D) Cu/Zn$^{2+}$ //Zn/ Cu$^{2+}$. Show Answer Correct Answer: C) Zn/Zn$^{2+}$ // Cu$^{2+}$/Cu. 40. In the reaction:Fe + Cu$^{2+ }$ $\rightarrow$Fe$^{2+}$ + CuWhat is your cathode electrode? A) Fe. B) Cu. C) All the above. D) None of the above. Show Answer Correct Answer: B) Cu. 41. The reaction 2NaCl $\rightarrow$ 2Na + Cl$_{2}$ is an example of A) A reduction reaction, only. B) Both an oxidation and reduction reaction. C) An oxidation reaction, only. D) Neither an oxidation nor a reduction reaction. Show Answer Correct Answer: B) Both an oxidation and reduction reaction. 42. What is the role of the anode in an electrochemical cell? A) The anode is the electrode that generates heat during the reaction. B) The anode is the electrode where oxidation occurs and electrons are released. C) The anode is the part of the cell that stores energy for later use. D) The anode is where reduction occurs and electrons are absorbed. Show Answer Correct Answer: B) The anode is the electrode where oxidation occurs and electrons are released. 43. An electrolytic cell is a nonspontaneous process that converts A) Electrical energy to chemical. B) Chemical energy to electrical. C) Thermal energy to electrical. D) Electrical energy to thermal. Show Answer Correct Answer: A) Electrical energy to chemical. 44. In voltaic cells, the salt bridge is important to ..... 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. 45. In an electrochemical cell, the salt bridge is used to: A) Complete the circuit and allow the flow of ions. B) Provide a surface for the reaction. C) Measure the cell potential. D) Act as a catalyst. Show Answer Correct Answer: A) Complete the circuit and allow the flow of ions. 46. In a voltaic cell, electrons flow spontaneously from A) Salt bridge to anode. B) Cathode to anode. C) Anode to cathode. D) Salt bridge to cathode. Show Answer Correct Answer: C) Anode to cathode. 47. What are the advantages of fuel cells? A) High efficiency, low emissions, pollution-free, flexibility in fuel sources. B) Low efficiency, high emissions, noisy operation, limited fuel sources. C) High efficiency, high emissions, unlimited energy, limited fuel sources. D) High cost, high emissions, noisy operation, limited fuel sources. Show Answer Correct Answer: A) High efficiency, low emissions, pollution-free, flexibility in fuel sources. 48. Integral of dQ/T is independent of reversible path connecting between two points. A) True. B) False. C) All the above. D) None of the above. Show Answer Correct Answer: A) True. 49. Given:(i) Cu2+ + 2e-$\rightarrow$ Cu, Eo = 0.337 V(ii) Cu2+ + e-$\rightarrow$ Cu+, Eo = 0.153 VElectrode potential E$^\circ$ for the reaction Cu+ + e-$\rightarrow$ Cu will be A) 0.184v. B) 0.380v. C) 0.530v. D) 0.284v. Show Answer Correct Answer: C) 0.530v. 50. In a voltaic cell, the electrode that is more easily oxidized is the ..... A) Anode. B) Anion. C) Cathode. D) Cation. Show Answer Correct Answer: A) Anode. 51. Ag+(aq) + e-$\rightarrow$ Ag(s) E$^\circ$ = + 0.80 VFe2+(aq)+ + 2e-$\rightarrow$ Fe(s) E$^\circ$ =-0.44 VWhat is emf ofFe(s) + 2Ag+(aq) $\rightarrow$ Fe2+(aq) + 2Ag(s) A) 1.16V. B) 2.04V. C) 1.24V. D) -1.16V. Show Answer Correct Answer: C) 1.24V. 52. Assume that the following reaction proceeds in an voltaic cell. If the concentration of Ag$^{+1}$ (aq) is 0.10M and the concentration of Au$^{+3}$ (aq) is 1.0M, what is the expected voltage from this reaction?Ag(s) + Au$^{+3}$ (aq) $\rightarrow$ Ag$^{+1}$ (aq) + Au(s)Ag$^{+1}$ + e$^{-}$ = Ag E$^\circ$ = +0.799VAu$^{+3}$ + 3e$^{-}$ = Au E$^\circ$ = +1.50V A) Less than 0.70 V. B) More than 0.70 V. C) Exactly 0.70 V. D) None of the above. Show Answer Correct Answer: B) More than 0.70 V. 53. An electrolytic cell is used to plate silver from a silver nitrate solution onto an electrode. How much time (in seconds) is required to deposit 8.0 g of silver if the current is kept constant at 5.0 amperes? Assume 100% current efficiency. (F = 96480 C/mol e$^{-}$) A) 2.5 x 10$^{4}$ s. B) 2.6 x 10$^{5}$ s. C) 1.4 x 10$^{3}$ s. D) 1.7 x 10$^{2}$ s. Show Answer Correct Answer: C) 1.4 x 10$^{3}$ s. 54. Two electrodes are fitted in conductance cell 1.5 cm apart while the area of cross section of each electrode is 0.75 cm$^{2}$. The cell constant is- A) 0.5 cm. B) 1.125. C) 2.0 cm$^{-1}$. D) 0.2 cm$^{-1}$. Show Answer Correct Answer: C) 2.0 cm$^{-1}$. 55. What is the significance of the salt bridge in a galvanic cell? A) The salt bridge acts as a barrier to stop electron flow. B) The salt bridge is used to generate heat in the cell. C) The salt bridge prevents ion flow to maintain charge separation. D) The salt bridge allows ion flow to maintain charge balance and enables continuous electron flow. Show Answer Correct Answer: D) The salt bridge allows ion flow to maintain charge balance and enables continuous electron flow. 56. Ionic compounds do not conduct electricity when they are solid because, A) Their electrons are not free to move. B) Their electrons are free to move. C) Their ions are free to move. D) Their ions are not free to move. Show Answer Correct Answer: D) Their ions are not free to move. 57. WHAT IS ELECTROCHEMISTRY A) THE INTERCONNECTION BETWEEN ELECTRICITY AND CHEMISTRY. B) FORMATION OF ELECTROLYTE. C) TO CELEBRATE GRACE. D) ELECTRICITY PASSING THROUGH A CHEMISTRY CLASS. Show Answer Correct Answer: A) THE INTERCONNECTION BETWEEN ELECTRICITY AND CHEMISTRY. 58. It is impossible to measure the half cell potential because A) The electron must be allowed to flow. B) Of the resistance offered by the solution. C) Ions are not free to move. D) There is no measuring device connected. Show Answer Correct Answer: A) The electron must be allowed to flow. 59. What is the primary purpose of a galvanic cell? A) To convert chemical energy into electrical energy. B) To facilitate chemical reactions without energy conversion. C) To store electrical energy. D) To measure electrical potential. Show Answer Correct Answer: A) To convert chemical energy into electrical energy. 60. Which of the following is a common application of electrochemistry in everyday life? A) Photosynthesis in plants. B) Batteries in electronic devices. C) Evaporation of water. D) Magnetic resonance imaging. Show Answer Correct Answer: B) Batteries in electronic devices. ← 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