This quiz works best with JavaScript enabled. Home > Class 12 > Class 12 Chemistry (Part I) Chapter 3 Electrochemistry – Quiz 11 🏠 Homepage 📘 Download PDF Books 📕 Premium PDF Books Class 12 Chemistry (Part I) Chapter 3 Electrochemistry Quiz 11 (25 MCQs) Quiz Instructions Select an option to see the correct answer instantly. 1. In the reaction:Fe + Cu$^{2+ }$ $\rightarrow$Fe$^{2+}$ + CuWhat is your anode electrode? A) Fe. B) Cu. C) All the above. D) None of the above. Show Answer Correct Answer: A) Fe. 2. What happens at the anode and cathode in a galvanic cell? A) No reaction at either the anode or cathode. B) Oxidation at both the anode and cathode. C) Oxidation at the anode and reduction at the cathode. D) Reduction at the anode and oxidation at the cathode. Show Answer Correct Answer: C) Oxidation at the anode and reduction at the cathode. 3. Define electrolysis and its applications. A) Electrolysis is primarily used for cooking food. B) Electrolysis is a method for generating electricity from solar panels. C) Electrolysis is only applicable in the textile industry. D) Electrolysis is used in various applications including electroplating, purification of metals, production of chemical compounds (like chlorine and hydrogen), and in water splitting for hydrogen fuel production. Show Answer Correct Answer: D) Electrolysis is used in various applications including electroplating, purification of metals, production of chemical compounds (like chlorine and hydrogen), and in water splitting for hydrogen fuel production. 4. What is the role of a salt bridge in a galvanic cell? A) To allow the flow of electrons between the two half-cells. B) To maintain electrical neutrality by allowing the flow of ions. C) To increase the voltage of the cell. D) To separate the two half-cells. Show Answer Correct Answer: B) To maintain electrical neutrality by allowing the flow of ions. 5. Nernst equation FOR (i) Mg(s) | Mg2+(0.001M) || Al3+(0.0001 M) | Al(s) A) E$_{CELL}$=E$^{0}$$_{CELL}$-0.0591/6 log[Mg2+]$^{3}$/[Al3+]$^{2}$. B) E$_{CELL}$=E$^{0}$$_{CELL}$-0.0591/6 log[Al3+]$^{2}$/[Mg2+]$^{3}$. C) E$_{CELL}$=E$^{0}$$_{CELL+}$0.0591/3 log[Mg2+]$^{3}$/[Al3+]$^{2}$. D) E$_{CELL}$=E$^{0}$$_{CELL}$-0.0591/3 log[Mg2+] /[Al3+]. Show Answer Correct Answer: A) E$_{CELL}$=E$^{0}$$_{CELL}$-0.0591/6 log[Mg2+]$^{3}$/[Al3+]$^{2}$. 6. Which of the following is true about an electrolyte?I Electrolyte conducts electricity in molten state.II Electrolyte conducts electricity in solid state.III Electrolyte is soluble in water.IV Electrolyte undergoes chemical decomposition when it conducts electricity. A) I and II only. B) II and III only. C) II and IV only. D) I and IV only. Show Answer Correct Answer: D) I and IV only. 7. Silver chloride can conduct electrocity in molten state, but not conducting in solid state. This is because silver chloride A) Is a covalent compound. B) Exist as freely moving charged particles in molten state. C) Exist as atoms in solid state. D) Has freely moving electrons in molten state. Show Answer Correct Answer: B) Exist as freely moving charged particles in molten state. 8. The correct relation between Avogadro's number and Faraday's constant is: A) W= EIt/F. B) F= WIt/E. C) F= WItE. D) W= FIt/E. Show Answer Correct Answer: A) W= EIt/F. 9. Consider the following half equation:Br$_{2}$(l) + 2e$^{-}$ $\rightarrow$ 2Br$^{-}$ (aq) E$^{0}$ = +1.07 VFe$^{2+}$ (aq) + 2e$^{-}$ $\rightarrow$ Fe(s) E$^{0}$ =-0.44 Vwhich of the following is a correct statement. A) Fe$^{2+}$ is a stronger reducing agent than Br$^{-}$. B) Fe is a stronger reducing agent than Br$_{2}$. C) Fe is a stronger reducing agent than Br$^{-}$. D) Fe is stronger reducing agent than Fe$^{2+}$. Show Answer Correct Answer: C) Fe is a stronger reducing agent than Br$^{-}$. 10. Electrical energy is produced in a voltaic cell by a ..... redox reaction within the cell. A) Nonspontaneous. B) Spontaneous. C) All the above. D) None of the above. Show Answer Correct Answer: B) Spontaneous. 11. Compare and contrast the functions of the anode and cathode in electrochemical cells. A) The anode and cathode both accept electrons through reduction. B) The anode accepts electrons through reduction, while the cathode releases electrons through oxidation. C) The anode releases electrons through oxidation, while the cathode accepts electrons through reduction. D) The anode and cathode both release electrons through oxidation. Show Answer Correct Answer: C) The anode releases electrons through oxidation, while the cathode accepts electrons through reduction. 12. Which electrode in a galvanic cell is positive? A) Anode. B) Cathode. C) Both are equally positive. D) Neither, as they are both neutral. Show Answer Correct Answer: B) Cathode. 13. In a concentration cell, how does the Nernst equation explain the generation of voltage? A) Voltage is generated due to the concentration gradient between two half-cells. B) Voltage is generated by the temperature difference between electrodes. C) Voltage is generated by the pressure difference in the cell. D) Voltage is generated by the presence of a catalyst. Show Answer Correct Answer: A) Voltage is generated due to the concentration gradient between two half-cells. 14. Which change occurs at the anode in an operating electrochemical cell? A) Gain of protons. B) Gain of electrons. C) Loss of protons. D) Loss of electrons. Show Answer Correct Answer: D) Loss of electrons. 15. What is the role of a cathode and anode in electrochemical reactions? A) The anode is where reduction occurs and gains electrons. B) The anode is where oxidation occurs and loses electrons, while the cathode is where reduction occurs and gains electrons. C) Both the anode and cathode are sites of oxidation. D) The anode gains electrons while the cathode loses electrons. Show Answer Correct Answer: B) The anode is where oxidation occurs and loses electrons, while the cathode is where reduction occurs and gains electrons. 16. Which of the following is a real-world application of electrochemistry? A) Photosynthesis in plants. B) Combustion engines. C) Batteries and fuel cells. D) Nuclear reactors. Show Answer Correct Answer: C) Batteries and fuel cells. 17. List some common applications of electrochemistry in daily life. A) Solar panels. B) Batteries, electroplating, corrosion prevention, electrolysis. C) Wind turbines. D) Hydraulic systems. Show Answer Correct Answer: B) Batteries, electroplating, corrosion prevention, electrolysis. 18. What is electrode potential? A) Electrode potential is the measure of the amount of ions in an electrode when in contact with a solution of its own ions. B) Electrode potential is the measure of the temperature of an electrode. C) Electrode potential is the measure of the color of an electrode. D) Electrode potential is the measure of the tendency of an electrode to gain or lose electrons in contact with a solution of its own ions. Show Answer Correct Answer: D) Electrode potential is the measure of the tendency of an electrode to gain or lose electrons in contact with a solution of its own ions. 19. In a galvanic cell, which component is responsible for the flow of electrons? A) Salt bridge. B) Electrolyte solution. C) Anode. D) Cathode. Show Answer Correct Answer: D) Cathode. 20. Electronic conduction is due to flow of A) Protons. B) Electrons. C) Neutrons. D) Ions. Show Answer Correct Answer: B) Electrons. 21. What are redox reactions and how do they occur? A) Redox reactions do not involve any changes in oxidation states. B) Redox reactions are chemical reactions where one substance is oxidized and another is reduced, involving the transfer of electrons. C) Redox reactions are limited to reactions in acidic solutions only. D) Redox reactions only involve the formation of new compounds without electron transfer. Show Answer Correct Answer: B) Redox reactions are chemical reactions where one substance is oxidized and another is reduced, involving the transfer of electrons. 22. The difference between the electrode potentials of two electrodes when no current is drawn through the cell is called ..... A) Cell potential. B) Potential difference. C) Cell voltage. D) Cell emf. Show Answer Correct Answer: D) Cell emf. 23. Which of the following is a primary cell? A) Lead-acid battery. B) Nickel-cadmium battery. C) Dry cell. D) Lithium-ion battery. Show Answer Correct Answer: C) Dry cell. 24. Because copper is not easily oxidized, it is often used as the ..... in voltaic cells. A) Cathode. B) Anode. C) Ion. D) Electrolyte bridge. Show Answer Correct Answer: A) Cathode. 25. The half-reaction that occurs at the anode during the electrolysis of molten sodium bromide is? A) 2 Br$^{-}$$\rightarrow$ Br$_{2}$ + 2 e$^{-}$. B) Br$_{2}$ + 2 e$^{-}$ $\rightarrow$ 2 Br$^{-}$. C) Na$^{+}$ + e$^{-}$ $\rightarrow$ Na. D) Na $\rightarrow$ Na$^{+}$ + e$^{-}$. Show Answer Correct Answer: A) 2 Br$^{-}$$\rightarrow$ Br$_{2}$ + 2 e$^{-}$. ← 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 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 8Class 12 Chemistry (Part I) Chapter 3 Electrochemistry Quiz 9Class 12 Chemistry (Part I) Chapter 3 Electrochemistry Quiz 10 🏠 Back to Homepage 📘 Download PDF Books 📕 Premium PDF Books