This quiz works best with JavaScript enabled. Home > Class 12 > 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 (25 MCQs) Quiz Instructions Select an option to see the correct answer instantly. 1. Which metal will spontaneously react with Zn$^{2+}$(aq), but will not spontaneously react with Mg$^{2+}$(aq)? A) Mn. B) Cu. C) Ni. D) Ba. Show Answer Correct Answer: A) Mn. 2. What is the purpose of the salt bridge in electrolytic cells? A) To supply additional electrolytes. B) To generate electricity. C) To prevent the electrodes from touching. D) Electrolytic cells do not use a salt bridge. Show Answer Correct Answer: D) Electrolytic cells do not use a salt bridge. 3. What are the products of electrolysis of water? A) Hydrogen and Oxygen. B) Sodium and Chlorine. C) Hydrogen Peroxide and Methane. D) Nitrogen and Carbon Dioxide. Show Answer Correct Answer: A) Hydrogen and Oxygen. 4. Calculate E for the following electrochemical cell at 25$^\circ$CPt | H$_{2}$(g) (1.0 atm) | H$^{+}$ (0.010 M) || Ag$^{+}$ (0.020 M) | Agif E$^\circ$ (H$^{+}$) = +0.000 V and E$^\circ$ (Ag$^{+}$) = 0.799 V A) +0.275 V. B) +0.799 V. C) +0.911 V. D) +0.817 V. Show Answer Correct Answer: C) +0.911 V. 5. Terminal positif sel elektrolisis A) Anion. B) Kation. C) Anod. D) Katod. Show Answer Correct Answer: C) Anod. 6. The molar conductivity of a 0.5 mol/dm$^{3}$ solution of AgNO3 with specific conductance of 5.76 x 10$^{-3}$ S cm$^{-1}$ at 298 K is A) 2.88 S cm$^{2}$/ mol. B) 11.52 S cm$^{2}$/ mol. C) 0.086 S cm$^{2}$/ mol. D) 28.8 S cm$^{2}$/ mol. Show Answer Correct Answer: B) 11.52 S cm$^{2}$/ mol. 7. Which of the following statements is(are) true for all voltaic (or galvanic) cells?(I) Reduction occurs at the cathode(II) The anode gains mass during discharge (note:this means operation of the cell.)(III) The voltage is less than or equal to zero. A) Only III. B) II and III. C) Only II. D) Only I. Show Answer Correct Answer: D) Only I. 8. What is the Nernst equation used for in electrochemistry? A) To calculate the equilibrium constant of a reaction. B) To determine the cell potential under non-standard conditions. C) To measure the pH of a solution. D) To find the concentration of ions in a solution. Show Answer Correct Answer: B) To determine the cell potential under non-standard conditions. 9. What occurs to the mass of zinc electrode in the following reaction?Zn/Zn+2 // Ag+1 / Ag A) Increases. B) Decreases. C) Remains the same. D) None of the above. Show Answer Correct Answer: B) Decreases. 10. How does the Nernst equation relate to concentration cells? A) It shows that cell potential is independent of concentration. B) It indicates that cell potential is directly proportional to concentration. C) It demonstrates that cell potential is inversely proportional to concentration. D) It explains how cell potential varies with concentration differences. Show Answer Correct Answer: D) It explains how cell potential varies with concentration differences. 11. Reactions in electrolytic cells are A) Spontaneous, redox reactions. B) Non-spontaneous, redox reactions. C) Spontaneous, non-redox reactions. D) Non-spontaneous, non-redox reactions. Show Answer Correct Answer: B) Non-spontaneous, redox reactions. 12. What factors influence the rate of electrolysis? A) Humidity levels in the environment. B) Type of light used during the process. C) Presence of magnetic fields. D) Factors influencing the rate of electrolysis include electrolyte type, concentration, temperature, electrode surface area, applied voltage, and electrode material. Show Answer Correct Answer: D) Factors influencing the rate of electrolysis include electrolyte type, concentration, temperature, electrode surface area, applied voltage, and electrode material. 13. If a conductivity and conductance of a solution is same then it's cell constant A) 1. B) 0. C) 10. D) 1000. Show Answer Correct Answer: A) 1. 14. Standard Conditions Galvanic Cells would be A) 1.0 M solutions. B) 1 atm pressure. C) 25$^{o}$ Celsius. D) All of the above. Show Answer Correct Answer: D) All of the above. 15. Specific conductance decreases with A) Decrese in concentration. B) Increse in concentration. C) Remains constant. D) None. Show Answer Correct Answer: A) Decrese in concentration. 16. In electrolytic cells, the cathode is characterized by: A) Oxidation. B) Reduction. C) Neutralization. D) Precipitation. Show Answer Correct Answer: B) Reduction. 17. The efficiency of a salt bridge is primarily due to its ability to: A) Increase the voltage of the cell. B) Conduct electrons between the half-cells. C) Maintain the charge balance by ion exchange. D) Store excess energy produced by the cell. Show Answer Correct Answer: C) Maintain the charge balance by ion exchange. 18. Which of the following reactions shows that copper is oxidized? A) Reaction of magnesium with copper (II)oxide. B) Reaction of copper with silver nitrate solution. C) Electrolysis of copper (II) nitratesolution by using carbon nitrate. D) Voltaic cell with copper and magnesiumelectrodes in dilute sulphuric acid. Show Answer Correct Answer: B) Reaction of copper with silver nitrate solution. 19. Which atom forms an ion that would migrate toward the cathode in an electrolytic cell? A) F. B) I. C) Na. D) Cl. Show Answer Correct Answer: C) Na. 20. Which of the following substances does not conduct electricity? A) Crystalline NaCl. B) Graphite. C) CuSO4 solution. D) NaCl crystals with a defect. Show Answer Correct Answer: A) Crystalline NaCl. 21. Why electrolytes in the solid state cannot conduct electricity? A) Solid state needs current with a high voltage. B) Solid state does not have free-moving ions. C) Solid state has a fixed shape. D) Solid state has a fixed volume. Show Answer Correct Answer: B) Solid state does not have free-moving ions. 22. How is voltage related to Gibbs free energy in electrochemical reactions? A) Voltage is directly proportional to Gibbs free energy. B) Voltage is equal to Gibbs free energy. C) Voltage is unrelated to Gibbs free energy. D) Voltage is inversely proportional to Gibbs free energy. Show Answer Correct Answer: A) Voltage is directly proportional to Gibbs free energy. 23. What factors affect the rate of electrolysis? A) Type of light used during the process. B) Time of day when electrolysis is performed. C) Factors affecting the rate of electrolysis include electrolyte type, concentration, temperature, electrode surface area, applied voltage, and electrode material. D) Size of the container holding the electrolyte. Show Answer Correct Answer: C) Factors affecting the rate of electrolysis include electrolyte type, concentration, temperature, electrode surface area, applied voltage, and electrode material. 24. How many moles of aluminum metal can be deposited when 0.600 moles of electrons are passed through 4.00 moles of molten Al$_{2}$O$_{3}$? A) 0.100. B) 0.200. C) 1.33. D) 1.80. Show Answer Correct Answer: B) 0.200. 25. In the galvanic cell in which the reaction Zn(s)+2Ag+(aq) $\rightarrow$Zn2+(aq)+2Ag(s)takes place. (i) Which of the electrode is negatively charged? A) Zn. B) Ag. C) Cathode. D) Salt bridge. Show Answer Correct Answer: A) Zn. ← 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 10Class 12 Chemistry (Part I) Chapter 3 Electrochemistry Quiz 11 🏠 Back to Homepage 📘 Download PDF Books 📕 Premium PDF Books