NEET Chemistry Equilibrium MCQs Set 01

Question:  The K_c 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 (K_p) are related as

• a)

  

• b)

  

• c)

  

• d)

  

Answer:

Question: In which of the following does the reaction go almost to completion?

• a) K_c= 10³ 
• b) K_c= 10²
• c) K_c= 10^–2
• d) K_c= 10^–3

Answer: K_c= 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:  K_p is how many times equal to K_c 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 K_p 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 K_p 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 K_p 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 K_c 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, K_p , for the reaction  is 1.8 × 10^–3 atm. The value of K_c 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 K_a 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, K_w= 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) K_h= K_w/K_a
• b) K_h= K_w/K_b
• c) K_h= K_w/K_a.K_b 
• d) K_h= K_w.K_a 

Answer: K_h= K_w/K_b

Question:  The solubility product of AgCl is K_sp . Then the solubility of AgCl in xM KCl is

• a)

  

• b)

  

• c)

  

• d)

  

Answer:

Question:  The correct representation for the K_sp of SnS₂ is

• a) [Sn²⁺][S^2–]²
• b) [Sn⁴⁺][S^–2]²
• c) [Sn²⁺][2S^–2]
• d) [Sn⁴⁺][2S^2–]²

Answer:  [Sn⁴⁺][S^–2]²

Question:  The K_sp 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 K_SP
• b) Exceeds K_SP
• c) Less than K_SP
• d) Is very small

Answer: Exceeds K_SP

Question:  The precipitate of CaF₂(K_sp= 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 K_C 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 K_p 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 K_p

• 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 K_c 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) K_c= 0.1 mol lt^–1
• b)

  

• c)

  

• d) K_p= 8 atm

Answer:  K_p= 8 atm