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Class 11 chemistry MCQ Question of Equilibrium with Answers?

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Practice Class 11 Chemistry MCQ Questions of Equilibrium with Answers consistently and score well in examinations. We have gathered the NCERT MCQ Questions for Class 11 Chemistry with Answers covering all topics of the syllabus. Refer to the Equilibrium Class 11 MCQ Questions with Answers here alongside a definite clarification.  Practice MCQ Questions, it makes you feel confident in answering the question in the exam & increases your scores to high.

Chemical equilibrium relates to such a state when the reactants, as well as products, will no longer undergo any further change. In such a case, the rate of forwarding and backward reaction remains the same. The concept of equilibrium becomes important for students to grasp advanced topics. Class 11 Chemistry equilibrium MCQ Questions provide a clear discussion on it.

Practice MCQ Questions for class 11 Chemistry Chapter-Wise

1. Which of the following aqueous solutions will have highest pH?

(a) NaCl
(b) CH3COONa
(c) Na2CO3
(d) NH4Cl

2. Which of the following oxides is not expected to react with sodium hydroxide?

(a) CaO
(b) SiO2
(c) BeO
(d) B2O3

3. The pH of a 10-10 M NaOH solution is nearest to

(a) 10
(b) 7
(c) 4
(d) -10

4. In a reversible chemical reaction at equilibrium, if the concentration of any one of the reactants is doubled, then the equilibrium constant will

(a) Also be Doubled
(b) Be Halved
(c) Remain the Same
(d) Become One-Fourth

5. When a neutral atom undergoes oxidation, the atoms oxidation state

(a) Decreases as it gains electrons
(b) Decreases as it loses electrons
(c) Increases as it gains electrons
(d) Increases as it loses electrons

6. Among the following the weakest Bronsted base is

(a) F
(b) Cl
(c) Br
(d) I

7. Among the following hydroxides, the one which has the lowest value of Ksp at ordinary temperature (about 25° ​​C ) is

(a) Mg (OH)2
(b) Ca(OH)2
(c) Ba(OH)2
(d) Be(OH)2

8. Amines behave as

(a) Lewis Acids
(b) Lewis Base
(c) Aprotic Acid
(d) Neutral Compound

9. Which of the following is not a general characteristic of equilibria involving physical processes?

(a) All the physical processes stop at equilibrium
(b) The opposing processes occur at the same rate and there is dynamic but stable condition
(c) All measurable properties of the system remain constant
(d) Equilibrium is possible only in a (closed system at a given temperature

10. Boiling point of the liquid depends on the atmospheric pressure. It depends on the altitude of the place; at high altitude the boiling point…………..

(a) decreases
(b) increases
(c) either decreases or increases
(d) remains same

11. Reaction is said to be in equilibrium when

(a) the rate of transformation of reactant to products is equal to the rate of transformation of products to the reactants.
(b) 50% of the reactants are converted to products
(c) the volume of reactants is just equal to the volume of the products
(d) the reaction is near completion and all the reactants are converted to products

12. Which of the following is not true about a reversible reaction?

(a) Number of moles of reactants and products is always equal
(b) It can be attained only in a closed container
(c) It cannot be influenced by a catalyst
(d) The reaction does not proceed to completion

13. If a system is at equilibrium, the rate of forward to the reverse reaction is

(a) equal
(b) less
(c) high
(d) at equilibrium

14. On doubling P and V with constant temperature the equilibrium constant will

(a) remain constant
(b) become one-fourth
(c) become double
(d) None of these 

15. Suitable conditions for melting of ice

(a) high temperature and high pressure
(b) high temperature and low pressure
(c) low temperature and low pressure
(d) low temperature and high pressure

16. What happens when an inert gas is added to an equilibrium keeping volume unchanged?

(a) More product will form
(b) Less product will form
(c) More reactant will form
(d) Equilibrium will remain unchanged

17. Which of the following statement(s) about the Arrhenius equation is incorrect?

(a) If Ea = 0,then k = A
(b) When the activation energy of the reaction is high, the rate becomes independent of temperature.
(c) Two reactions having same value of Ea do not necessarily have same rate.
(d) A reaction with higher value of Ea will have smaller value of rate constant.

18. A base, as defined by Bronsted theory, is a substance which can

(a) accept protons
(b) gain a pair of electrons
(c) donate protons
(d) lose a pair of electrons

19. Which among the following salt solutions is basic in nature?

(a) Ammonium chloride
(b) Ammonium sulphate
(c) Ammonium nitrate
(d) Sodium acetate

20. The pH of 0.01 M NaOH (aq) solution will be-

(a) 7.01
(b) 2
(c) 12
(d) 9

21. Boric acid is an  acid because its molecule

(a) contains replaceable H+ ion
(b) gives up a proton
(c) accepts OH- from water releasing proton
(d) combines with proton from water molecule

22. Which of the following fluoro-compounds is most likely to behave as a Lewis base?

(a) BF3
(b) PF3
(c) CF4
(d) SiF4

23. Among the following, the correct order of acidity is

(a) HClO < HClO2 < HClO3 < HClO4
(b) HClO2 < HClO < HClO3 < HClO4
(c) HClO4 < HClO2 < HClO < HClO3
(d) HClO3 < HClO4 < HClO2 < HClO

24. Consider the nitration of benzene using mixed conc. H2SO4 and HNO3. If a large amount of KHSO4 is added to the mixture, the rate of nitration will be

(a) slower 
(b) unchanged
(c) doubled
(d) faster

25. Aqueous solution of which of the following compounds is the best conductor of electric current?

(a) Ammonia, NH3
(b) Fructose,C6H12O6
(c) Acetic acid, C2H4O2
(d) Hydrochloric acid, HCl

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Answer:

1. Answer : (c) Na2CO3

Explanation: The hydrolysis of NaCl gives neutral solution because it is salt of strong acid and strong base and hence, its PH is 7. NH4Cl is salt of weak base and strong acid, so its PH is less than 7. NaHCO3 is also acidic whereas Na2CO3 is salt of strong base and weak acid, so its PH is more than 7.

2. Answer : (a) CaO

Explanation: CaO being a basic oxide does not react with NaOH, however SiO2 (acidic oxide), BeO (amphoteric oxide) and Br2O3 (acidic oxide) react with NaOH.

3. Answer : (c) 4

Explanation: pOH= −log [OH]

= −log 10-10

= 10 log 10

= 10pH + pOH

= 14pH

= 14−pOH

= 14−10

= 4

4. Answer : (c) Remain the Same

Explanation: Equilibrium constant is independent of the concentration of reactants.

5. Answer : (d) Increases as it loses electrons

Explanation: The acronym “OILRIG” can be used to remember this: Oxidation is Losing electrons, Reduction is Gaining electrons. Therefore, when an atom undergoes oxidation, it loses electrons. This makes its net charge more positive, so its oxidation state increases.

6. Answer : (d) I

Explanation: According to this theory, an acid is a proton donor and a base is a proton acceptor. Every strong Bronsted acid has a weak conjugate base and every strong base has a weak conjugate acid. The acidity increases in halogen group atoms, HF < HCl < HBr < HI. So, HI is highly acidic and their conjugate bases decrease in order F– > Cl > Br > I.

7. Answer : (d) Be(OH)2

Explanation: Be(OH)2 ​has the lowest value of Ksp at ordinary temperature because Be2+ ion is smaller than the other metal ions in the group, which results in a tighter bond with the OH ions, thus much lower solubility.The solubility of a hydroxide of group 2 elements increases down the group because as you go down the group size of metal increases thereby increasing the bond length and decreasing bond energy.

8. Answer : (b) Lewis Base

Explanation: The substance which can donate a pair of| electrons is called Lewis base.Amines contain a lone pair of electron on| nitrogen atom, so behave as Lewis base.

9. Answer : (a) All the physical processes stop at equilibrium

Explanation: A physical equilibrium is dynamic in nature, both forward and reverse process occur at equal rates. The some kind of motion is always present. The individual molecules continuously move from one phase to another.

10. Answer : (a) decreases

Explanation: At higher altitudes, there is less atmospheric pressure, and so it takes less energy (lower temperature) for liquids to boil.

11. Answer : (a) the rate of transformation of reactant to products is equal to the rate of transformation of products to the reactants.

Explanation: A reaction is said to be in equilibrium when rate of forward reaction is equal to the rate of backward reaction.

12. Answer : (a) Number of moles of reactants and products is always equal

Explanation: In a reversible reaction, number of moles of reactants and products is not always equal.It is attained only if the system is closed.A catalyst does not alter the equilibrium point. It alters the rate of the reaction. The equilibrium can be shifted either to left or right by altering the volume, pressure, temperature etc.

13. Answer : (a) equal

Explanation: At equilibrium, the rate of forward & backward reaction become equal.

14. Answer : (a) remain constant

Explanation: On doubling P and volume with constant T, the equilibrium constant (K) will remain constant. Temperature always changes K because on adding heat to a system in state of equilibrium will always alter the forward reaction rate differently than the reverse reaction rate.

15. Answer :(a) high temperature and high pressure

Explanation: Since ice has lower density than water, melting of ice involves reduction in volume. Increase in pressure favours the process. The process is endothermic and hence high temperature favours the process.

16. Answer : (d) Equilibrium will remain unchanged

Explanation: On adding inert gas at constant volume the total pressure of the system is increased, but the partial pressure of each reactant and product remains the same. Hence no effect on the state of equilibrium.

17. Answer : (b) When the activation energy of the reaction is high, the rate becomes independent of temperature.

Explanation: When the activation energy of the reaction is high, the rate becomes independent of temperature.

18. Answer : (a) accept protons

Explanation: According to Bronsted theory, acid is a substance that can release protons while base are those that accept protons.

19. Answer :(d) Sodium acetate

Explanation: CH3COONa ⇒ Salt of CH3COOH(WA) + NaOH(SB)

∴ Solution of CH3COONa shows basic nature

20. Answer : (c) 12

Explanation: NaOH(aq) is strong base solution

So, [OH−] = N = 10−2N

pOH = −log[OH− ]=−log10−2 = 2

pH = 14 − pOH = 14 − 2

pH = 12

21. Answer : (c) accepts OH- from water releasing proton

Explanation: Boric acid is an acid because its molecule accepts OH from water releasing proton. The reaction is as follows:

B(OH)3 + H2\(\leftrightharpoons\)​ [B(OH)4]- + H+​​​​​​

22. Answer : (b) PF3

Explanation: PF3 → Lewis base (presence of lone pair on p atom)

23. Answer : (a) HClO < HClO< HClO3 < HClO4

Explanation: Acidic strength ∝ EN ∝ + ve Oxidation state.

24. Answer : (a) slower 

Explanation: If a large amount of KHSO4 is added then conc. of HSO-4 ions increases and the reaction will be shifted in backward direction hence, the rate of nitration will be slower.

25. Answer : (d) Hydrochloric acid, HCl

Explanation: Aqueous solution of HCl is the best conductor of electric current because HCl is strong acid, so it dissociates completely into ions.

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