This quiz works best with JavaScript enabled. Home > Class 12 > Class 12 Chemistry (Part I) Chapter 3 Electrochemistry – Quiz 3 🏠 Homepage 📘 Download PDF Books 📕 Premium PDF Books Class 12 Chemistry (Part I) Chapter 3 Electrochemistry Quiz 3 (25 MCQs) Quiz Instructions Select an option to see the correct answer instantly. 1. In a redox reaction how doe the number of electrons lost compare to the number of electrons gained? A) The number lost is sometimes equal to the number gained. B) The number lost is always equal to the number gained. C) The number lost is always greater than the number gained. D) The number lost is always less than the number gained. Show Answer Correct Answer: B) The number lost is always equal to the number gained. 2. An electrochemical cell can behave like an electrolytic cell when A) E$_{cell }$= 0. B) E$_{cell}$> E$_{ext}$. C) E$_{ext}$> E$_{cell}$. D) E$_{cell }$= E$_{ext}$. Show Answer Correct Answer: C) E$_{ext}$> E$_{cell}$. 3. Given the equation representing a reaction:Cd + NiO$_{2}$ + 2H$_{2}$O Cd(OH)$_{2}$ + Ni(OH)$_{2}$Which half-reaction equation represents the oxidation in the reaction? A) Ni$^{4+}$ + 2e$^{-}$ Ni$^{2+}$. B) Ni$^{4+}$ Ni$^{2+}$ + 2e$^{-}$. C) Cd Cd$^{2+}$ + 2e$^{-}$. D) Cd + 2e$^{-}$ Cd$^{2+}$. Show Answer Correct Answer: C) Cd Cd$^{2+}$ + 2e$^{-}$. 4. The positive value of the standard electrode potential of Cu+2/Cu indicates that A) This redox couple is a stronger reduction agent than the H/H2 couple. B) This redox couple is a stronger oxidizing agent than H+/H2. C) Cu cannot displace H2 from acid. D) None. Show Answer Correct Answer: B) This redox couple is a stronger oxidizing agent than H+/H2. 5. Describe the process of electrolysis and its applications. A) Electrolysis is primarily used for cooking food. B) Electrolysis is a method of painting surfaces. C) Electrolysis is used in various applications including electroplating, metal extraction, water splitting for hydrogen production, and the purification of metals. D) Electrolysis is only applicable in the textile industry. Show Answer Correct Answer: C) Electrolysis is used in various applications including electroplating, metal extraction, water splitting for hydrogen production, and the purification of metals. 6. Pt | MnO$_{4}$$^{-}$, Mn$^{2+}$ | | Zn$^{2+}$ | ZnFor the cell above, identify the cathode and anode. A) Cathode:MnO$_{4}$$^{-}$Anode:Zn. B) Cathode:ZnAnode:Pt. C) Cathode:ZnAnode:MnO$_{4}$$^{-}$. D) Cathode:PtAnode:Zn. Show Answer Correct Answer: B) Cathode:ZnAnode:Pt. 7. An anion is ..... charged ion. A) Positively. B) Neutrally. C) Negatively. D) None of the above. Show Answer Correct Answer: C) Negatively. 8. What is a reduction? A) Loss of electrons. B) Gain of electrons. C) Loss of mass. D) Gain of mass. Show Answer Correct Answer: B) Gain of electrons. 9. According to Ohm's Law, If to the ends of a conductor, a voltage 'E' is applied and a current 'I' flows through it, then the resistance 'R' A) E x I. B) I/E. C) E/I. D) None of the above. Show Answer Correct Answer: C) E/I. 10. According to Faraday's first law, the amount of substances produced or consumed at cathode or anode electrode is directly proportional to the A) Voltage provided. B) Concentration of electrolyte. C) Quantity of electricity passed. D) Temperature of solution. Show Answer Correct Answer: C) Quantity of electricity passed. 11. What is the difference between primary and secondary cells? A) Primary cells are rechargeable; secondary cells are non-rechargeable. B) Both primary and secondary cells are rechargeable. C) Primary cells can be reused; secondary cells cannot. D) Primary cells are non-rechargeable; secondary cells are rechargeable. Show Answer Correct Answer: D) Primary cells are non-rechargeable; secondary cells are rechargeable. 12. In the zinc-copper voltaic cell, electrons are produced at the ..... A) Cathode. B) Anode. C) All the above. D) None of the above. Show Answer Correct Answer: B) Anode. 13. It is the method that can be used for both qualitative and quantitative analysis of a wide variety of molecular and ionic materials. A) Voltammetry. B) Potentiometry. C) Ammetry. D) Electrometry. Show Answer Correct Answer: A) Voltammetry. 14. What is the role of a salt bridge in an electrochemical cell? A) To maintain electrical neutrality. B) To increase the cell potential. C) To act as a catalyst. D) To provide a surface for the reaction. Show Answer Correct Answer: A) To maintain electrical neutrality. 15. Cell potential is proportional to the slope of the Gibbs energy with respect to the extent of the reaction. A) True. B) False. C) All the above. D) None of the above. Show Answer Correct Answer: A) True. 16. In the reaction:Fe + Cu$^{2+ }$ $\rightarrow$Fe$^{2+}$ + CuWhich half-reaction can be found in the anode? A) Fe + 2e$^{-}$ $\rightarrow$ Fe$^{2+}$. B) Fe $\rightarrow$ Fe$^{2+ }$+ 2e$^{-}$. C) Cu$^{2+}$$\rightarrow$Cu + 2e$^{-}$. D) Cu$^{2+ }$+ 2e$\rightarrow$ Cu. Show Answer Correct Answer: B) Fe $\rightarrow$ Fe$^{2+ }$+ 2e$^{-}$. 17. Which of the following is a common method to prevent corrosion? A) Heating the metal. B) Applying a protective coating. C) Exposing the metal to acids. D) Keeping the metal in a vacuum. Show Answer Correct Answer: B) Applying a protective coating. 18. In the anode, the metal strip will gradually ..... A) Increase in size. B) Decrease in size. C) Stay the same size. D) Dissolve completely. Show Answer Correct Answer: B) Decrease in size. 19. Calculate standard cell potential for this equation:Zn$^{2+}$(aq) + 2e $\rightarrow$ Zn(s) E$^\circ$ =-0.76 VCd$^{2+}$(aq) + 2e $\rightarrow$ Cd(s) E$^\circ$ =-0.40 V A) E$^{o}$cell =-0.36 V. B) E$^{o}$cell =-1.16 V. C) E$^{o}$cell = +1.16 V. D) E$^{o}$cell = +0.36 V. Show Answer Correct Answer: D) E$^{o}$cell = +0.36 V. 20. Is it possible for a cell potential to have NEGATIVE sign? A) NO. B) YES. C) All the above. D) None of the above. Show Answer Correct Answer: A) NO. 21. The substance that is oxidized is referred to as a oxidizing agent. A) True. B) False. C) All the above. D) None of the above. Show Answer Correct Answer: B) False. 22. Given the balanced ionic equation representing a reaction:2Al(s) + 3Cu$^{+2}$$\rightarrow$ 2Al$^{+3}$+ 3Cu(s) Which half-reaction represents the reduction that occurs? A) Al$\rightarrow$ Al$^{+3}$+3e. B) Al$^{+3}$+3e $\rightarrow$ Al. C) Cu$\rightarrow$ Cu$^{+2}$+2e. D) Cu$^{+2}$+ 2e $\rightarrow$ Cu. Show Answer Correct Answer: D) Cu$^{+2}$+ 2e $\rightarrow$ Cu. 23. The standard reduction potentials of X, Y, Z metals are 0.52, -3.03, -1.18 respectively. The order of reducing power of the corresponding metals is A) Y>Z>X. B) X>Y>Z. C) Z>Y>X. D) Z>X>Y. Show Answer Correct Answer: A) Y>Z>X. 24. It is a branch of chemistry that deals with interconversion between chemical and electrical energy. This process involves redox reaction. A) Electromagnetism. B) Electrochemistry. C) Electronic Chemistry. D) None of the choices. Show Answer Correct Answer: B) Electrochemistry. 25. One Faraday is: A) The amount of charge carried by 1 mole of electrons. B) The amount of charge carried by 1g of electrons. C) The amount of charge carried by 1 electron. D) The amount of charge carried by 1 Kg of electron. Show Answer Correct Answer: A) The amount of charge carried by 1 mole of electrons. ← PreviousNext →Related 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 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 8Class 12 Chemistry (Part I) Chapter 3 Electrochemistry Quiz 9Class 12 Chemistry (Part I) Chapter 3 Electrochemistry Quiz 10Class 12 Chemistry (Part I) Chapter 3 Electrochemistry Quiz 11 🏠 Back to Homepage 📘 Download PDF Books 📕 Premium PDF Books