This quiz works best with JavaScript enabled. Home > Class 12 > Class 12 Chemistry (Part I) Chapter 3 Electrochemistry – Quiz 23 🏠 Homepage 📘 Download PDF Books 📕 Premium PDF Books Class 12 Chemistry (Part I) Chapter 3 Electrochemistry Quiz 23 (25 MCQs) Quiz Instructions Select an option to see the correct answer instantly. 1. In a voltaic cell, electrons flow spontaneously from A) Cathode to anode. B) Salt bridge to anode. C) Salt bridge to cathode. D) Anode to cathode. Show Answer Correct Answer: D) Anode to cathode. 2. What are the advantages of fuel cells? A) High efficiency, low emissions, pollution-free, flexibility in fuel sources. B) High efficiency, high emissions, unlimited energy, limited fuel sources. C) High cost, high emissions, noisy operation, limited fuel sources. D) Low efficiency, high emissions, noisy operation, limited fuel sources. Show Answer Correct Answer: A) High efficiency, low emissions, pollution-free, flexibility in fuel sources. 3. 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. 4. 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) 0.284v. B) 0.530v. C) 0.184v. D) 0.380v. Show Answer Correct Answer: B) 0.530v. 5. In a voltaic cell, the electrode that is more easily oxidized is the ..... A) Anode. B) Cathode. C) Anion. D) Cation. Show Answer Correct Answer: A) Anode. 6. 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) 1.24V. C) 2.04V. D) -1.16V. Show Answer Correct Answer: B) 1.24V. 7. 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. 8. 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) 1.7 x 10$^{2}$ s. B) 1.4 x 10$^{3}$ s. C) 2.5 x 10$^{4}$ s. D) 2.6 x 10$^{5}$ s. Show Answer Correct Answer: B) 1.4 x 10$^{3}$ s. 9. 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) 1.125. B) 0.5 cm. C) 2.0 cm$^{-1}$. D) 0.2 cm$^{-1}$. Show Answer Correct Answer: C) 2.0 cm$^{-1}$. 10. . The charge required for the reduction of 1 mol of MnO4-to MnO2 is A) 1F. B) 3F. C) 5 F. D) 6 F. Show Answer Correct Answer: B) 3F. 11. 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. 12. Ionic compounds do not conduct electricity when they are solid because, A) Their electrons are not free to move. B) Their ions are free to move. C) Their ions are not free to move. D) Their electrons are free to move. Show Answer Correct Answer: C) Their ions are not free to move. 13. 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. 14. 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. 15. What is the primary purpose of a galvanic cell? A) To facilitate chemical reactions without energy conversion. B) To measure electrical potential. C) To store electrical energy. D) To convert chemical energy into electrical energy. Show Answer Correct Answer: D) To convert chemical energy into electrical energy. 16. Which of the following is a common application of electrochemistry in everyday life? A) Batteries in electronic devices. B) Photosynthesis in plants. C) Evaporation of water. D) Magnetic resonance imaging. Show Answer Correct Answer: A) Batteries in electronic devices. 17. A group of cells that are connected together A) Anode. B) Battery. C) Salt bridge. D) Half cell. Show Answer Correct Answer: B) Battery. 18. Alkaline battery is an example of A) Primary cells. B) Secondary cells. C) Fuel cells. D) Electrolytic cells. Show Answer Correct Answer: A) Primary cells. 19. 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. 20. Oxidation state A) The apparent charge of a particle. B) Anion. C) Cation. D) Reduction. Show Answer Correct Answer: A) The apparent charge of a particle. 21. 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) 4OH-O2 + 2H2O + 4e-. B) Al3+ + 3e-Al. C) Al Al3+ + 3e-. D) 2O2-O2 + 4e-. Show Answer Correct Answer: B) Al3+ + 3e-Al. 22. 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. 23. 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. 24. Which metal have highest reducing power.Given the standard electrode potentials, A) K+/K =-2.93V,. B) Ag+/Ag = 0.80V,. C) Hg2+/Hg = 0.79V. D) Mg2+/Mg =-2.37 V,. E) Cr3+/Cr =-0.74V. Show Answer Correct Answer: A) K+/K =-2.93V,. 25. 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. ← 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