Equilibrium Class 11 MCQ is one of the best strategies to prepare for the CBSE Class 11 Board exam. If you want to complete a grasp concept or work on one’s score, there is no method except constant practice. Students can improve their speed and accuracy by doing more MCQs on Equilibrium Class 11, which will help them all through their board tests.
Equilibrium Class 11 MCQ Question with Answer
Class 11 Chemistry MCQ with answers are given here to Chapter 7 Equilibrium. These MCQs are based on the latest CBSE board syllabus and relate to the latest Class 11 Chemistry syllabus. By Solving these Class 11 MCQs, you will be able to analyze all of the concepts quickly in the chapter and get ready for the Class 11 Annual exam.
Learn Class 11 Equilibrium MCQs with answers pdf free download according to the latest CBSE and NCERT syllabus. Students should prepare for the examination by solving CBSE Class 11 Chemistry Equilibrium MCQ with answers given below
Question 1. The values of Kp1 and Kp2 for the reactions, X ⇌ Y + Z …(i) A ⇌ 2B …(ii) are in the ratio 9 : 1. If degree of dissociation of X and A be equal, then total pressure at equilibrium (i) and ii) are in the ratio
(a) 36 : 1
(b) 1 : 1
(c) 3 : 1
(d) 1 : 9
Question 2. If the concentration of OH– ions in the reaction Fe(OH)3(s) ⇌ Fe3+(aq) + 3OH– (aq) is decreased by 1/4 times, then equilibrium concentration of Fe3+ will increase by
(a) 64 times
(b) 4 times
(c) 8 times
(d) 16 times.
Question 3. In liquid-gas equilibrium, the pressure of vapours above the liquid is constant at
(a) constant temperature
(b) low temperature
(c) high temperature
(d) none of these.
Question 4. The reaction, 2A(g) + B(g) ⇌ 3C(g) + D(g) is begun with the concentrations of A and B both at an initial value of 1.00 M. When equilibrium is reached, the concentration of D is easured and found to be 0.25 M. The value for the equilibrium constant for this reaction is given by the expression
(a) [(0.75)3(0.25)] ÷ [(1.00)2(1.00)]
(b) [(0.75)3(0.25)] ÷ [(0.50)2(0.75)]
(c) [(0.75)3(0.25)] ÷ [(0.50)2(0.25)]
(d) [(0.75)3(0.25)] ÷ [(0.75)2(0.25)]
Question 5. Which of the following statements is correct for a reversible process in a state of equilibrium?
(a) ΔG° = –2.30 RT log K
(b) ΔG° = 2.30 RT log K
(c) ΔG = –2.30 RT log K
(d) ΔG = 2.30 RT log K
Question 6. Which one of the following conditions will favour maximum formation of the product in the reaction A2(g) + B2(g) ⇌ X2(g), ΔrH = –X kJ ?
(a) Low temperature and high pressure
(b) Low temperature and low pressure
(c) High temperature and high pressure
(d) High temperature and low pressure
Question 7. If the value of equilibrium constant for a particular reaction is 1.6 × 1012, then at equilibrium the system will contain
(a) mostly products
(b) similar amounts of reactants and products
(c) all reactants
(d) mostly reactants.
Question 8. In Haber process, 30 litres of dihydrogen and 30 litres of dinitrogen were taken for reaction which yielded only 50% of the expected product. What will be the composition of aseous mixture under the aforesaid condition in the end?
(a) 20 litres ammonia, 20 litres nitrogen, 20 litres hydrogen
(b) 10 litres ammonia, 25 litres nitrogen, 15 litres hydrogen
(c) 20 litres ammonia, 10 litres nitrogen, 30 litres hydrogen
(d) 20 litres ammonia, 25 litres nitrogen, 15 litres hydrogen
Question 9. For the reversible reaction, N2(g) + 3H2(g) ⇌ 2NH3(g) + heat The equilibrium shifts in forward direction
(a) by increasing the concentration of NH3(g)
(b) by decreasing the pressure
(c) by decreasing the concentrations of N2(g) and H2(g)
(d) by increasing pressure and decreasing emperature.
Question 10. KMnO4 can be prepared from K2MnO4 as per the reaction,3MnO4 2– + 2H2O ⇌ 2MnO4 – + MnO2 + 4OH– The reaction can go to completion by removing OH– ions by dding
Question 11. For any reversible reaction, if we increase concentration of the reactants, then effect onequilibrium constant
(a) depends on amount of concentration
Question 12. A 20 litre container at 400 K contains CO2(g) at pressure 0.4 atm and an excess of SrO (neglect the volume of solid SrO). The volume of the container is now decreased by moving he movable piston fitted in the container. The maximum volume of the container, when pressure of CO2 attains its maximum value, will be (Given that : SrCO3(s) ⇌ SrO(s) + O2(g), Kp = 1.6 atm)
(a) 10 litre
(b) 4 litre
(c) 2 litre
(d) 5 litre
Question 13. In which of the following equilibrium Kc and Kp are not equal?
(a) 2NO(g) ⇌ N2(g) + O2(g)
(b) SO2(g) + NO2(g) ⇌ SO3(g) + NO(g)
(c) H2(g) + I2(g) ⇌ 2HI(g)
(d) 2C(s) + O2(g) ⇌ 2CO2(g)
Question 14. Aqueous solution of which of the following compounds is the best conductor of electric current?
(a) Hydrochloric acid, HCl
(b) Ammonia, NH3
(c) Fructose, C6H12O6
(d) Acetic acid, C2H4O2
Question 15. Aqueous solution of acetic acid contains
(a) CH3COO– and H+
(b) CH3COO–, H3O+ and CH3COOH
(c) CH3COO–, H3O+ and H+
(d) CH3COOH, CH3COO– and H+
Question 16. According to Le Chatelier’s principle, adding heat toa solid and liquid in equilibrium will cause the
(a) temperature to increase
(b) temperature to decrease
(c) amount of liquid to decrease
(d) amount of solid to decrease.
Question 17. Which one of the following information can be obtained on the basis of Le Chatelier principle?
(a) Dissociation constant of a weak acid
(b) Entropy change in a reaction
(c) Equilibrium constant of a chemical reaction
(d) Shift in equilibrium position on changing value of a constraint
Question 18. The pH of a 0.1 M solution of NH4 OH (having Kb = 1.0 x 10-5 ) is equal to
Question 19. The pH ofa solution obtained by mixing 50 mL of 1 N HCl and 30 mL of 1 N NaOH is (log 2.5 = 0.3979)
Question 20. Conjugate base for Bronsted acids H2O and HF are
(a) H3O+ and H2F+, respectively
(b) OH– and H2F+, respectively
(c) H3O+ and F–, respectively
(d) OH– and F–, respectively.
Question 21. The value of DH for the reaction X2(g) + 4Y2(g) ⇌ 2XY4(g) is less than zero.Formation of XY4(g) will be favoured at
(a) high temperature and high pressure
(b) low pressure and low temperature
(c) high temperature and low pressure
(d) high pressure and low temperature.
Question 22. Which of the following solutions will have pH = 9 at 298 K?
(a) 1 X 10-9 M HCl solution
(b) 1 x 10-5 M NaOH solution
(c) 1 X 10-9 M KOH solution
(d) Both (a) and (b)
Question 23. pH of a 0.0001 M HCI solution is
(b) 2 .0
(c) 6 .0
Question 24. pH of an aqueous solution containing 10-8 mol /L of HCI is
Question 25. Calculate the pH of a solution in which hydrogen ion concentration is 0.005 g-equi /L.
(b) 2 .8
(c) 2 .9
Question 26. The approximately pH of0.005 molar sulphw·ic acid is
Question 27. 100 mL of 0.015 M HCI solution is mixed with 100 mL of 0.005 M HCI. What is the pH of the resultant solution?
Question 28. Hydroxyl ion concentration of 10-2 M HCl is
(a) 1 x 101 mol dm-3
(b) 1 x 10-12 mol dm-3
(c) 1 x 10-1 mol dm-3
(d) 1 x 10-14 mol dm-3
Question 29. 100 mL of 0.01 M solution of NaOH is diluted to 1dm3 . What is the pH of the diluted solution?
Question 30. Calculate pOH of 0.001 M NH4OH, when it is 1% dissociated in the solution.
Question 31. What will be the pH value of0.05M Ba (OH)2 solution?
Question 32. Which solution has pH equal to 10?
(a) 10-4 M KOH
(b) 10-10 M KOH
(c) 10-10 M HCI
(d) 10-4 M HCl
Whoever needs to take the CBSE Class 11 Board Exam should look at this MCQ. To the Students who will show up in CBSE Class 11 Chemistry Board Exams, It is suggested to practice more and more questions. Aside from the sample paper you more likely had solved. These Equilibrium Class 11 MCQ are ready by the subject specialists themselves.
Question 33. A 0.01 M ammonia solution is 5% ionised, its pH will be
(d) 12 .24
Question 34. Which of the following cannot act both as Bronsted acid and as Bronsted base ?
(a) HCO3 –
(d) HSO– 4
Question 35. The pH value of 1/1000 N KOH solution is
Question 36. Reaction BaO2(s) ⇌ BaO(s) + O2(g); ΔH = +ve. In equilibrium condition, pressure of O2 depends on
(a) increase mass of BaO2
(b) increase mass of BaO
(c) increase temperature on equilibrium
(d) increase mass of BaO2 and BaO both.
Question 37. Which of the following molecules acts as a Lewis acid?
Question 38. Which one of the following statements is not true?
(a) Among halide ions, iodide is the most powerful reducing agent.
(b) Fluorine is the only halogen that does not show a variable oxidation state.
(c) HOCl is a stronger acid than HOBr.
(d) HF is a stronger acid than HCl.
Question 39. Which one of the following compounds is not a protonic acid?
Question 40. Which of the following fluoro-compounds is mostlikely to behave as a Lewis base?
Question 41. Which is the strongest acid in the following?
Question 42. Which one of the following molecular hydrides acts as a Lewis acid?
Question 43. The strongest conjugate base is
(a) SO4 2–
(c) NO3 –
Question 44. Which of the following is not a Lewis acid?
Question 45. Repeated use of which one of the following fertilizers would increase the acidity of the soil?
(a) Ammonium sulphate
(b) Superphosphate of lime
(d) Potassium nitrate
Question 46. Which of these is least likely to act as a Lewis base?
Question 47. In HS–, I–, R – NH2, NH3 order of proton accepting tendency will be
(a) I– > NH3 > R – NH2 > HS–
(b) NH3 > R – NH2 > HS– > I–
(c) R – NH2 > NH3 > HS– > I–
(d) HS– > R – NH2 > NH3 > I–
Question 48. Conjugate acid of NH2 – is
(b) NH4 +
(c) NH2 –
Question 49. Which compound is electron deficient?
Question 50. Find out the solubility of Ni(OH)2 in 0.1 M NaOH. Given that the ionic product of Ni(OH)2 is 2 × 10–15.
(a) 2 × 10–13 M
(b) 2 × 10–8 M
(c) 1 × 10–13 M
(d) 1 × 108 M
Question 51. The pH of 0.01 M NaOH(aq) solution will be
Question 52. At 100°C the Kw of water is 55 times its value at 25°C. What will be the pH of neutral solution? (log 55 = 1.74)
Question 53. Equimolar solutions of the following substances were prepared separately. Which one of these will record the highest pH value?
Question 54. The percentage of pyridine (C5H5N) that forms pyridinium ion (C5H5N + H) in a 0.10 M aqueous pyridine solution (Kb for C5H5N = 1.7 × 10–9) is
Question 55. Accumulation of lactic acid (HC3H5O3), a monobasic acid in tissues leads to pain and a feeling of fatigue. In a 0.10 M aqueous solution, lactic acid is 3.7% dissociated. The value of issociation constant, Ka, for this acid will be
(a) 1.4 × 10–5
(b) 1.4 × 10–4
(c) 3.7 × 10–4
(d) 2.8 × 10–4
Question 56. What is the pH of the resulting solution when equal volumes of 0.1 M NaOH and 0.01 M HCl are mixed?
Question 57. Which of the following salts will give highest pH in water?
Question 58. What is [H+] in mol/L of a solution that is 0.20 M in CH3COONa and 0.10 M in CH3COOH? (Ka for CH3COOH = 1.8 × 10–5)
(a) 3.5 × 10–4
(b) 1.1 × 10–5
(c) 1.8 × 10–5
(d) 9.0 × 10–6
Question 59. The ionization constant of ammonium hydroxide is 1.77 × 10–5 at 298 K. Hydrolysis constant of ammonium chloride is
(a) 6.50 × 10–12
(b) 5.65 × 10–13
(c) 5.65 × 10–12
(d) 5.65 × 10–10
Question 60. The hydrogen ion concentration of a 10–8 M HCl aqueous solution at 298 K (Kw = 10–14) is
(a) 1.0 × 10–8 M
(b) 1.0 × 10–6 M
(c) 1.0525 × 10–7 M
(d) 9.525 × 10–8 M
Question 61. At 25°C, the dissociation constant of a base, BOH, is 1.0 × 10–12. The concentration of hydroxyl ions in 0.01 M aqueous solution of the base would be
(a) 1.0 × 10–5 mol L–1
(b) 1.0 × 10–6 mol L–1
(c) 2.0 × 10–6 mol L–1
(d) 1.0 × 10–7 mol L–1
Question 62. What is the [OH–] in the final solution prepared by mixing 20.0 mL of 0.050 M HCl with 30.0 mL of 0.10 M Ba(OH)2?
(a) 0.40 M
(b) 0.0050 M
(c) 0.12 M
(d) 0.10 M
Question 63. Which has highest pH?
Question 64. Ionisation constant of CH3COOH is 1.7 × 10–5 and concentration of H+ ions is 3.4 × 10–4. Then find out initial concentration of CH3COOH molecules.
(a) 3.4 × 10–4
(b) 3.4 × 10–3
(c) 6.8 × 10–4
(d) 6.8 × 10–3
Question 65. Calculate the pOH of a solution at 25°C that contains 1 × 10–10 M of hydronium ions, i.e. H3O+.
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Frequently Asked Question (FAQs)
How many MCQ questions are there in Class 11 chapter 7 Chemistry?
In Class 11 chapter 7 Chemistry, we have provided 65 Important MCQ Questions, But in the future, we will add more MCQs so that you can get good marks in the Class 11 exam.
Can we score good marks in Class 11 Chemistry with the help of Equilibrium MCQ Questions?
Yes, MCQ Question is one of the best strategies to make your preparation better for the CBSE Board Exam. It also helps to know the student’s basic understanding of each chapter. So, You can score good marks in the Class 11 Chemistry exam.