Refer to NEET Chemistry Equilibrium MCQs Set A provided below available for download in Pdf. The MCQ Questions for Full Syllabus Chemistry with answers are aligned as per the latest syllabus and exam pattern suggested by NEET, NCERT and KVS. Multiple Choice Questions for Equilibrium are an important part of exams for Full Syllabus Chemistry and if practiced properly can help you to improve your understanding and get higher marks. Refer to more Chapter-wise MCQs for NEET Full Syllabus Chemistry and also download more latest study material for all subjects
MCQ for Full Syllabus Chemistry Equilibrium
Full Syllabus Chemistry students should refer to the following multiple-choice questions with answers for Equilibrium in Full Syllabus.
Equilibrium MCQ Questions Full Syllabus Chemistry with Answers
Question: The Kc for given reaction will be
- a)
- b)
- c)
- d)
Answer:
Question: For which of the following reaction, the degree of dissociation (α and equilibrium constant (Kp) are related as
- a)
- b)
- c)
- d)
Answer:
Question: In which of the following does the reaction go almost to completion?
- a) Kc= 103
- b) Kc= 102
- c) Kc= 10–2
- d) Kc= 10–3
Answer: Kc= 103
Question: In a chemical equilibrium the rate constant of the backward reaction is 7.5 × 10–4 and the equilibrium constant is 1.5. So the rate constant of the forward reaction is
- a) 2 × 10–3
- b) 15 × 10–4
- c) 1.125 × 10–3
- d) 9.0 × 10–4
Answer: 1.125 × 10–3
Question: Kp is how many times equal to Kc for the given reaction?
- a)
- b) R2T2
- c)
- d) RT
Answer:
Question: 4 g H2, 32 g O2, 14 g N2 and 11g CO2 are taken in a bulb of 500 ml. Which one of these has maximum active mass?
- a) H2
- b) O2
- c) N2
- d) CO2
Answer: H2
Question: For reaction, will be
- a) x
- b)
- c)
- d)
Answer:
Question: XY2 dissociates as,
Initial pressure of XY2 is 600 mm Hg. The total pressure at equilibrium is 800 mm Hg. Assuming volume of system to remain constant, the value of Kp is
- a) 50
- b) 100
- c) 20
- d) 400
Answer: 100
Question: The initial pressure of COCl2 is 1000 torr. The total pressure of the system becomes 1500 torr, when the equilibrium
is attained at constant temperature. The value of Kp of a reaction
- a) 1500
- b) 1000
- c) 2500
- d) 500
Answer: 500
Question: Hydrogen (a moles) and iodine (b moles) react to give 2x moles of the HI at equilibrium. The total number of moles at equilibrium is
- a) a + b + 2x
- b) (a – b) + (b – 2x)
- c) (a + b)
- d) a + b – x
Answer: (a + b)
Question: When ethyl alcohol and acetic acid mixed together in equimolecular proportions, equilibrium is attained when two–third of the acid and alcohol are consumed. The equilibrium constant of the reaction will be
- a) 0.4
- b) 4
- c) 40
- d) 0.04
Answer: 4
Question: Two moles of N2 and two moles of H2 are taken in a closed vessel of 5 litres capacity and suitable conditions are provided for the reaction. When the equilibrium is reached, it is found that a half mole of N2 is used up. The equilibrium concentration of NH3 is
- a) 0.3
- b) 0.4
- c) 0.2
- d) 0.1
Answer: 0.2
Question: 1 mole of NO2 and 2 moles of CO are enclosed in a one litre vessel to attain the following equilibrium NO2+
It was estimated that at the equilibrium, 25% of initial amount of CO is consumed. The equilibrium constant Kp is
- a) 1
- b) 1/2
- c) 1/4
- d) 1/3
Answer: 1/3
Question: Two moles of NH3 gas are introduced into a previously evacuated one litre vessel in which it partially dissociates at high temperature as
At equilibrium, one mole of NH3(g) remain.The value of Kc is
- a) 3
- b) 27/16
- c) 3/2
- d) 27/64
Answer: 27/16
Question: 15. 4.0 moles of PCl5 dissociate at 760 K in a 2 litre flask,
at equilibrium. 0.8 moleof Cl2 was present in the flask. The equilibrium constant would be
- a) 1.0 × 10–1
- b) 1.0 × 10–4
- c) 1.0 × 10–2
- d) 1.0 × 10–3
Answer: 1.0 × 10–1
Question: When 3.00 mole of A and 1.00 mole of B are mixed in a 1.00 litre vessel, the following reaction takes place
The equilibrium mixture contains 0.5 mole of C. What is the value of equilibrium constant for the reaction?
- a) 0.12
- b) 6
- c) 1.5
- d) 3
Answer: 0.12
Question: At 700 K, the equilibrium constant, Kp , for the reaction is 1.8 × 10–3 atm. The value of Kc for the above reaction at the same temperature in moles per litre would be
- a) 1.1 × 10–7
- b) 3.1 × 10–5
- c) 6.2 × 10–7
- d) 9.3 × 10–7
Answer: 3.1 × 10–5
Question: Which one of the following equilibrium moves backward when pressure is applied?
- a)
- b)
- c)
- d)
Answer:
Question: In melting of ice, which one of the conditions will be more favourable?
- a) High temperature and high pressure
- b) Low temperature and low pressure
- c) Low temperature and high pressure
- d) High temperature and low pressure
Answer: High temperature and high pressure
Question: Given the reaction,
Which combination of pressure and temperature gives the highest yield of Z at equilibrium?
- a) 1000 atm and 500°C
- b) 500 atm and 500°C
- c) 1000 atm and 100°C
- d) 500 atm and 100°C
Answer: 1000 atm and 100°C
Question: Calculate the percentage ionization of 0.01 M acetic acid in 0.1 M HCl Ka of acetic acid is 1.8 × 10–5
- a) 0.18%
- b) 0.018%
- c) 1.8%
- d) 18%
Answer: 0.018%
Question: A 0.2 molar solution of formic acid is 3.2% ionised, its ionisation constant is
- a) 9.6 × 10–3
- b) 2.1 × 10–4
- c) 1.25 × 10–6
- d) 2.1 × 10–8
Answer: 2.1 × 10–4
Question: At 100°C, Kw= 10–12. pH of pure water at 100°C will be
- a) 7.0
- b) 6.0
- c) 8.0
- d) 12.0
Answer: 6.0
Question: A monoprotic acid in a 0.1 M solution ionises to 0.001%. Its ionisation constant is
- a) 1.0 × 10–3
- b) 1.0 × 10–6
- c) 1.0 × 10–8
- d) 1.0 × 10–11
Answer: 1.0 × 10–11
Question: When 0.1 mole of ammonia is dissolved in sufficient water to make 1 litre of solution. The solution is found to have a hydroxide ion concentration of 1.34 × 10–3. The dissociation constant of ammonia is
- a) 1.8 × 10–5
- b) 1.6 × 10–6
- c) 1.34 × 10–3
- d) 1.8 × 10–4
Answer: 1.8 × 10–5
Question: A solution of NaOH contain 0.04 gm of NaOH per litre. Its pH is
- a) 10
- b) 9
- c) 11
- d) 12
Answer: 11
Question: 1 c.c of 0.1 N HCl is added to 1 litre solution of sodium chloride. The pH of the resulting solution will be
- a) 7
- b) 0
- c) 10
- d) 4
Answer: 4
Question: 100 c.c. of N/10 NaOH solution is mixed with 100 c.c. of N/5 HCl solution and the whole volume is made to 1 litre. The pH of the resulting solution will be
- a) 1
- b) 2
- c) 3
- d) 4
Answer: 2
Question: The pH of a solution is zero. The solution is
- a) Neutral
- b) Normal acid
- c) Decinormal acid
- d) Strongly alkaline
Answer: Normal acid
Question: 100 ml of 0.1 N NaOH is mixed with 100 ml of 0.1 N H2SO4 . The pH of the resultant solution is
- a) < 7
- b) > 7
- c) = 7
- d) Cannot be predicted
Answer: = 7
Question: The pH of 0.016 M NaOH solution is
- a) 1.796
- b) 12.204
- c) 11
- d) None of these
Answer: 12.204
Question: pH of 1 M HCl is
- a) Zero
- b) –2
- c) 7
- d) 14
Answer: Zero
Question: For a acid 'A' pH = 2 and for acid 'B' pH is 4. Then
- a) A is more basic than B
- b) B is more acidic than A
- c) A is more acidic than B
- d) B is more basic than A
Answer: A is more acidic than B
Question: The addition of solid sodium carbonate to pure water causes
- a) An increase in the hydronium ion concentration
- b) An increase in pH
- c) No change in pH
- d) A decrease in the hydroxide ion concentration
Answer: An increase in pH
Question: A buffer solution can be prepared from a mixture of
I. Sodium acetate and acetic acid in water
II. Sodium chloride and HCl in water
III. Ammonia and NH4Cl in water
IV. Ammonia and sodium hydroxide in water
- a) 1, 3, 4
- b) 2, 3, 4
- c) 1, 2, 4
- d) 1, 3
Answer: 1, 3
Question: A salt of strong acid and weak base is dissolved in water. Its hydrolysis in solution is
- a) Unaffected on heating
- b) Increased by adding strong acid
- c) Suppressed by diluting
- d) Suppressed by adding strong acid
Answer: Suppressed by adding strong acid
Question: The following reactions are known to occur in the body
If CO2 escapes from the system
- a) pH will decrease
- b) Hydrogen ion concentration will diminish
- c) H2CO3 concentration will be promoted
- d) The forward reaction will be promoted
Answer: Hydrogen ion concentration will diminish
Question: Which of the following salts undergoes hydrolysis?
- a) CH3COONa
- b) KNO3
- c) NaCl
- d) K2SO4
Answer: CH3COONa
Question: A 0.1 N solution of sodium bicarbonate has a pH value of
- a) 5.6
- b) 7.0
- c) 8.4
- d) 4.0
Answer: 8.4
Question: Which will undergo cationic hydrolysis?
- a) NaCl
- b) CH3COONa
- c) (NH4)2SO4
- d) H2CO3
Answer: (NH4)2SO4
Question: Degree of hydrolysis (h) of a salt of weak acid and a strong base is given by
- a)
- b)
- c)
- d)
Answer:
Question: pH of a salt of a strong base with weak acid
- a)
- b)
- c)
- d) None of these
Answer:
Question: Which relation is correct for NH4Cl?
- a) Kh= Kw/Ka
- b) Kh= Kw/Kb
- c) Kh= Kw/Ka.Kb
- d) Kh= Kw.Ka
Answer: Kh= Kw/Kb
Question: The solubility product of AgCl is Ksp . Then the solubility of AgCl in xM KCl is
- a)
- b)
- c)
- d)
Answer:
Question: The correct representation for the Ksp of SnS2 is
- a) [Sn2+][S2–]2
- b) [Sn4+][S–2]2
- c) [Sn2+][2S–2]
- d) [Sn4+][2S2–]2
Answer: [Sn4+][S–2]2
Question: The Ksp for a sparingly soluble Ag2CrO4 is 4 × 10–12. The molar solubility of the salt is
- a) 2.0 × 10–6 mol L–1
- b) 1.0 × 10–4 mol L–1
- c) 2.0 × 10–12 mol L–1
- d) 1.0 × 10–15 mol L–1
Answer: 1.0 × 10–4 mol L–1
Question: Precipitation occurs only if I.P (Ionic Product)
- a) Equals KSP
- b) Exceeds KSP
- c) Less than KSP
- d) Is very small
Answer: Exceeds KSP
Question: The precipitate of CaF2(Ksp= 1.7 × 10–10) is obtained when equal volumes of the following are mixed
- a) 10–4 M Ca2+ + 10–4 M F–
- b) 10–2 M Ca2+ + 10–3 M F–
- c) 10–4 M Ca2+ + 10–3 M F–
- d) 10–3 M Ca2+ + 10–5 M F–
Answer: 10–2 M Ca2+ + 10–3 M F–
Question: The equilibrium constant KC for the following reaction will be
- a)
- b)
- c)
- d)
Answer:
Question: At temperature T, a compound AB2(g) dissociates according to the reaction,
with a degree of dissociation 'x' which is small as compared to unity. The expression for Kp in terms of 'x' and total pressure P is
- a)
- b)
- c)
- d)
Answer:
Question: Ammonium carbamate dissociates as
In a closed vessel containing ammonium carbamate in equilibrium, ammonia is added such that the partial pressure of NH3 now equals to the original total pressure. The ratio of total pressure now to the original pressure is
- a)
- b)
- c)
- d)
Answer:
Question: When 1 mole of N2 and 1 mole of H2 is enclosed in 3L vessel and the reaction is allowed to attain equilibrium, it is found that at equilibrium there is 'x' mole of H2 . The number of moles of NH3 formed would be
- a)
- b)
- c)
- d)
Answer:
Question: 1 mole of 'A', 1.5 mole of 'B' and 2 mole of 'C' are taken in a vessel of volume one litre. At equilibrium concentration of C is 0.5 mole/L. Equilibrium constant for the reaction
- a) 0.66
- b) 0.066
- c) 66
- d) 6.6
Answer: 0.066
Question: The number of hydrogen ions in 10 ml of a solution with pH = 13 is
- a) 1013
- b) 6.023 × 108
- c) 6.023 × 1010
- d) 6.023 × 1013
Answer: 6.023 × 108
Question:
At the start of a reaction, there are 0.249 mol N2, 3.21 × 10–2 mol H2 and 6.42 × 10–4 mol NH3 in a 3.50 L reaction vessel at 375°C. Hence reaction will proceed in
- a) Forward direction
- b) Backward direction
- c) At equilibrium
- d) Stops
Answer: Forward direction
Question: Solid ammonium carbamate dissociated according to the given reaction
Total pressure of the gases in equilibrium is 5 atm. Hence Kp
- a) 18.5
- b) 25
- c) 1/ 5
- d) 12.5
Answer: 18.5
Question: 1.1 mole of A is mixed with 1.2 mol of B and the mixture is kept in a 1 L flask till the equilibrium
is reached. At equilibrium 0.1 mol of D is formed. The Kc of the reaction
- a) 0.002
- b) 0.004
- c) 0.001
- d) 0.003
Answer: 0.004
Question: In the following reaction
which pair can act as Bronsted bases only?
- a)
- b)
- c)
- d)
Answer:
Question: In the equilibrium
at 2000 K and 10 atm pressure, % Cl2= % SO2= 40 (byvolume) Then
- a) Kc= 0.1 mol lt–1
- b)
- c)
- d) Kp= 8 atm
Answer: Kp= 8 atm
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MCQs for Chemistry NEET Full Syllabus Equilibrium
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Equilibrium MCQs Chemistry NEET Full Syllabus
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Equilibrium NEET Full Syllabus MCQs Chemistry
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NEET MCQs Chemistry Full Syllabus Equilibrium
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