This quiz works best with JavaScript enabled. Home > Class 11 > Class 11 Chemistry (Part Ii) Chapter 8 Redox Reactions – Quiz 27 🏠 Homepage 📘 Download PDF Books 📕 Premium PDF Books Class 11 Chemistry (Part Ii) Chapter 8 Redox Reactions Quiz 27 (25 MCQs) Quiz Instructions Select an option to see the correct answer instantly. 1. Which of the following is a characteristic of a reduction process? A) Gain of electrons. B) Loss of electrons. C) Gain of protons. D) Loss of protons. Show Answer Correct Answer: A) Gain of electrons. 2. Which equation represents a redox reaction? A) NaOH + HNO$_{3 }$$\rightarrow$ NaNO$_{3}$ +H$_{2}$O. B) 2AgNO$_{3}$ + Zn $\rightarrow$ Zn(NO$_{3}$)$_{2}$ + 2Ag. C) 2NaCl + Pb(NO$_{3}$)$_{2}$ $\rightarrow$ PbCl$_{2}$ + 2NaNO$_{3}$. D) CaCO$_{3}$ + 2HCl $\rightarrow$ CaCl$_{2}$ + H$_{2}$O + CO$_{2}$. Show Answer Correct Answer: B) 2AgNO$_{3}$ + Zn $\rightarrow$ Zn(NO$_{3}$)$_{2}$ + 2Ag. 3. In the half-reaction $MnO_4^-\rightarrow Mn^{2+}$ A) +7 to +2. B) +2 to +7. C) +4 to +2. D) +2 to +4. Show Answer Correct Answer: A) +7 to +2. 4. Which of the following is used in the breathalyzer test to detect the presence of alcohol? A) Lime water. B) Lighter splint. C) Bromine water. D) Potassium dichromate. Show Answer Correct Answer: D) Potassium dichromate. 5. Why does aluminium tend not to corrode as much as iron when it is exposed to moist air? A) Aluminium does not lose electrons easily. B) A layer of aluminium oxide protects the metal beneath. C) Aluminium does not react with oxygen unless salt is present. D) Energy must be added to cause aluminium to corrode. Show Answer Correct Answer: B) A layer of aluminium oxide protects the metal beneath. 6. The iron (II) ion, Fe$^{2+}$(aq) A) Can act as an oxidant but not a reductant. B) Can oxidise solid zinc and reduce liquid bromine. C) Can act as a reductant but not an oxidant. D) Will always be reduced to Fe(s) in redox reactions. Show Answer Correct Answer: B) Can oxidise solid zinc and reduce liquid bromine. 7. What is the easier technique for balancing redox reactions under basic conditions? A) Use the neutralization method. B) Start with acidic conditions and then add hydroxide. C) Start with basic conditions and then add acid. D) Use the full reaction method. Show Answer Correct Answer: B) Start with acidic conditions and then add hydroxide. 8. The third step in balancing the redox reaction using oxidation-number-change is A) Check the balancing for both atoms and charge. B) Use coefficients to make the total increase in oxidation number equal to the total decrease in oxidation number. C) Assign oxidation numbers to each of the atoms in the equation and write the numbers above the atom. D) Use a line to connect the atoms that are undergoing a change in oxidation number. Show Answer Correct Answer: D) Use a line to connect the atoms that are undergoing a change in oxidation number. 9. What ions are present in molten aluminium oxide? A) Al$^{3+}$, O$^{2-}$, H$^{+}$, OH$^{-}$. B) Al$^{3+}$, O$^{2-}$. C) Al$^{3+}$, OH$^{-}$. D) None of the above. Show Answer Correct Answer: B) Al$^{3+}$, O$^{2-}$. 10. When a reactant loses hydrogen ..... A) Reduction reaction occur. B) Oxidation reaction occur. C) Hydrogenation occur. D) Combustion occur. Show Answer Correct Answer: B) Oxidation reaction occur. 11. Why is it important to balance both particles and charges in a redox reaction? A) To ensure conservation of mass. B) To ensure conservation of charge. C) To speed up the reaction. D) To simplify the equation. Show Answer Correct Answer: B) To ensure conservation of charge. 12. The ability of an atom to attract the bonding electrons to itself is defined as ..... A) Ionization energy. B) Ionic bond. C) Electronegativity. D) Electron affinity. Show Answer Correct Answer: C) Electronegativity. 13. How do you balance a half equation for a reaction? A) By changing the charge of ions. B) By adding or removing protons. C) By adding or removing electrons to balance charge. D) By adding spectator ions. Show Answer Correct Answer: C) By adding or removing electrons to balance charge. 14. $\Delta$H = + 300 kJ A) Endo. B) Exo. C) All the above. D) None of the above. Show Answer Correct Answer: A) Endo. 15. Which one of the following reactions is not a redox reaction? A) Zn(s) + CuSO$_{4}$(aq) $\rightarrow$ ZnSO$_{4}$(aq) + Cu(s). B) 2FeCl$_{2}$(s) + Cl$_{2}$(g) $\rightarrow$ 2FeCl$_{3}$(s). C) 2KI(aq) + Cl$_{2}$(g) $\rightarrow$ 2KCl(aq) + I$_{2}$(s). D) CaO(s) + 2HCl(aq) $\rightarrow$ CaCl$_{2}$(aq) + H$_{2}$O(l). Show Answer Correct Answer: D) CaO(s) + 2HCl(aq) $\rightarrow$ CaCl$_{2}$(aq) + H$_{2}$O(l). 16. What is the role of hydrogen ions in the reaction with magnesium? A) They precipitate out as a solid. B) They gain electrons and form hydrogen gas. C) They act as spectator ions. D) They lose electrons and form hydrogen gas. Show Answer Correct Answer: B) They gain electrons and form hydrogen gas. 17. What role do oxidation states play in chemistry? A) They determine the color of compounds. B) They indicate the temperature of a reaction. C) They measure the acidity of a solution. D) They simplify the tracking of electron sharing. Show Answer Correct Answer: D) They simplify the tracking of electron sharing. 18. Which of the following is the balanced half-reaction for the oxidation of Cu to Cu$^{+2?}$ A) Cu $\rightarrow$ Cu$^{+2}$. B) Cu + 2 e-$\rightarrow$ Cu$^{+2}$. C) Cu $\rightarrow$ Cu$^{+2 }$+ 2 e-. D) Cu-2e-$\rightarrow$ Cu$^{+2}$. Show Answer Correct Answer: C) Cu $\rightarrow$ Cu$^{+2 }$+ 2 e-. 19. What is the oxidation state of carbon in the reaction with silver diamine? A) +4. B) +3. C) +2. D) +1. Show Answer Correct Answer: A) +4. 20. The last step in balancing the redox reaction using oxidation-number change method is check the balancing for both atoms and charge. A) True. B) False. C) All the above. D) None of the above. Show Answer Correct Answer: A) True. 21. How many electrons are transferred in the reaction below?4Fe + 3O$_{2}$ $\rightarrow$ 2Fe$_{2}$O$_{3}$ A) 12 electrons. B) 6 electrons. C) 4 electrons. D) 3 electrons. Show Answer Correct Answer: A) 12 electrons. 22. What is the oxidation number of Chlorine in HClO4? A) +1. B) +3. C) +5. D) +7. Show Answer Correct Answer: D) +7. 23. In the reaction of hydrogen with iodine, which is the reducing agent? A) Hydrogen. B) Iodine. C) Hydrogen ion. D) Iodide ion. Show Answer Correct Answer: A) Hydrogen. 24. Explain the role of a salt bridge in an electrochemical cell. A) The role of a salt bridge in an electrochemical cell is to maintain electrical neutrality and allow ion flow between the half-cells. B) To increase the voltage of the cell. C) To prevent the flow of electrons. D) To act as a catalyst in the reaction. Show Answer Correct Answer: A) The role of a salt bridge in an electrochemical cell is to maintain electrical neutrality and allow ion flow between the half-cells. 25. In electrolytic cell which its electrolyte is aqueous copper (II) sulfate, copper are used as electrodes. What is the product at the anode? A) Oxygen gas and water. B) Copper metal. C) Copper (II) ions. D) Hydrogen gas. Show Answer Correct Answer: C) Copper (II) ions. ← PreviousNext →Related QuizzesClass 11 Chemistry (Part Ii) Chapter 8 Redox Reactions Quiz 1Class 11 Chemistry (Part Ii) Chapter 8 Redox Reactions Quiz 2Class 11 Chemistry (Part Ii) Chapter 8 Redox Reactions Quiz 3Class 11 Chemistry (Part Ii) Chapter 8 Redox Reactions Quiz 4Class 11 Chemistry (Part Ii) Chapter 8 Redox Reactions Quiz 5Class 11 Chemistry (Part Ii) Chapter 8 Redox Reactions Quiz 6Class 11 Chemistry (Part Ii) Chapter 8 Redox Reactions Quiz 7Class 11 Chemistry (Part Ii) Chapter 8 Redox Reactions Quiz 8Class 11 Chemistry (Part Ii) Chapter 8 Redox Reactions Quiz 9Class 11 Chemistry (Part Ii) Chapter 8 Redox Reactions Quiz 10 🏠 Back to Homepage 📘 Download PDF Books 📕 Premium PDF Books