Please refer to MCQ Questions Equilibrium for Chapter 7 Class 11 Chemistry given below. All MCQ questions are provided with answers. These MCQ Questions for Class 11 Chemistry are designed based on the chapters given in your CBSE NCERT Textbook for Class 11 Chemistry. These MCQ Questions are expected to come in your class 11 Board exams.
Question. 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. 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. 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. 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. 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. 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. 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. 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. 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. 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. 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. 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. For any reversible reaction, if we increase concentration of the reactants, then effect onequilibrium constant
(a) depends on amount of concentration
Question. 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. 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. 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. 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. 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. 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. The pH of a 0.1 M solution of NH4 OH (having Kb = 1.0 x 10-5 ) is equal to
Question. 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. pH of a 0.0001 M HCI solution is
(b) 2 .0
(c) 6 .0
Question. pH of an aqueous solution containing 10-8 mol /L of HCI is
Question. 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. 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. 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. Calculate the pH of a solution in which hydrogen ion concentration is 0.005 g-equi /L.
(b) 2 .8
(c) 2 .9
Question. The approximately pH of0.005 molar sulphw·ic acid is
Question. 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
Question. A 0.01 M ammonia solution is 5% ionised, its pH will be
(d) 12 .24
Question. 100 mL of 0.01 M solution of NaOH is diluted to 1dm3 . What is the pH of the diluted solution?
Question. Calculate pOH of 0.001 M NH4OH, when it is 1% dissociated in the solution.
Question. What will be the pH value of0.05M Ba (OH)2 solution?
Question. The pH value of 1/1000 N KOH solution is
Question. 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. Which of the following cannot act both as Bronsted acid and as Bronsted base ?
(a) HCO3 –
(d) HSO– 4
Question. Which is the strongest acid in the following?
Question. Which one of the following molecular hydrides acts as a Lewis acid?
Question. Which of the following molecules acts as a Lewis acid?
Question. 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. Which one of the following compounds is not a protonic acid?
Question. Which of the following fluoro-compounds is mostlikely to behave as a Lewis base?
Question. Which of these is least likely to act as a Lewis base?
Question. 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. The strongest conjugate base is
(a) SO4 2–
(c) NO3 –
Question. Which of the following is not a Lewis acid?
Question. 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. 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. The pH of 0.01 M NaOH(aq) solution will be
Question. Conjugate acid of NH2 – is
(b) NH4 +
(c) NH2 –
Question. Which compound is electron deficient?
Question. 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. 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. 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. Equimolar solutions of the following substances were prepared separately. Which one of these will record the highest pH value?
Question. 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. 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. What is the pH of the resulting solution when equal volumes of 0.1 M NaOH and 0.01 M HCl are mixed?
Question. Which of the following salts will give highest pH in water?
Question. 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. Calculate the pOH of a solution at 25°C that contains 1 × 10–10 M of hydronium ions, i.e. H3O+.
Question. 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. 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. Which has highest pH?
Question. 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