1st Year Chemistry Chapter 06 Chemical Equilibrium MCQs Quiz Test

If you are looking MCQs for 1st year Chapter Six "Chemical Equilibrium" MCQs Question Answers with solutions you are here on right website. On this Page you will learn Chapter Six objective type solved Questions with solutions. All of these chapter wise first Year Chemistry question answers are helpful for upcoming exams and tests preparations. These MCQs are also helpful for entry tests.

First Year Chemistry Chemical Equilibrium MCQs

You will learn in this Chapter:

• Reversible and Irreversible Reactions
• State of Chemical Equilibrium
• Law of mass action
• Equilibrium Constants
• Applications of Equilibrium Constants
• Le-Chatilier’s Principle
• Applications of Chemical Equilibrium in Industry
• Ionic Product of Water
• Ionization Constants of Acids/Base
• Lowry Bronsted Acid-Base Concept
• Common Ion Effect
• Buffer Solution
• Buffer Capacity
• Solubility Product

Q.1: What will be the pH of 1.0 mol dm^-3 of H₂X, which is only 50% dissociated??

1. 1
2. 0
3. 2
4. Less than 0

B

Q.2: What will be the pH of 1.0 mol dm^-3 of NH₄OH, which is 1% dissociated??

1. 2
2. 12
3. 0
4. 2.7

B

Q.3: Buffer solutions are used in except??

1. Clinical analysis
2. Nutrition
3. Soil science
4. Qualitative analysis

D

Q.4: Buffer action can be explained by except??

1. Common ion effect
2. Le-Chatelier’s principle
3. Law of mass action
4. Solubility product

D

Q.5: At equilibrium, the concentration of reactants and products are?

1. Constant
2. Maximum
3. Different
4. Equal

A

Q.6: In the reaction A_2(g) + 4B_2(g) ⇌ 2AB_4(g) such that ΔH < 0;the formation of AB_4(g)will be favoured at?

1. Low temperature and high pressure
2. High temperature and low pressure
3. Low temperature and low pressure
4. High temperature and high pressure

A

Q.7: Consider the reaction PCl_{5 (g)} ⇌ PCl_3(g) +Cl₂ in a closed container at equilibrium. At a fixed temperature, what will be the effect of adding more PCl₅ on the equilibrium constant??

1. It increases
2. It remains unaffected
3. It decreases
4. Can’t be predicted without K_P

B

Q.8: The oxidation of SO₂ to SO₃ is an exothermic reaction. The yield of SO₃ will be maximum if?

1. Temperature is increased and pressure is kept constant
2. Temperature is reduced and pressure is increased
3. Both temperature and pressure are increased
4. Both temperature and pressure are decreased

B

Q.9: If the concentration of salt is greater than the acid in buffer solution, then the??

1. pH = pK_a
2. pH = pK_b
3. pH > pK_a
4. pH > pK_b

A

Q.10: In a saturated solution of AgCl, the molar concentration of Ag⁺ and Cl^– is 1.0 x 10^-5 M each. What is the value of Ksp??

1. 1.0 x 10^-5
2. 0.1 x 10^-5
3. 1.0 x 10^-15
4. 1.0 x 10-¹⁰

D

Q.11: The solubility of Fe(OH)₃ is x molar per dm³. Its K_sp would be?

1. 9x³
2. 27x⁴
3. 3x⁴
4. 9x⁴

B

Q.12: For the reaction H_2(g) + I_2(g) ⇌ 2HI_(g). The equilibrium constant changes with?

1. Total pressure
2. The concentration of H₂ and I₂
3. Catalyst
4. Temperature

D

Q.13: The decomposition of N₂O₄ to NO₂ is carried out at 280°C in chloroform. When equilibrium is reached, 0.2 moles of N₂O₄ and 0.02 mole of NO₂ are present in 1:1 ratio. The equilibrium constant for the reaction N₂O₄ →2NO₂ is------.?

1. 0.01
2. 0.001
3. 0.02
4. 0.002

D

Q.14: In a given system, water and ice are in equilibrium, if the pressure is applied to the above system then?

1. More ice is formed
2. The amount of ice and water will remain the same
3. More ice is melted
4. Both a and b

C

Q.15: The solubility product of AgCl is 2.0 x 10^-10 mol²dm^-6. The maximum concentration of Ag⁺ ions in the solution is?

1. 1.41 x 10^-5 mol² dm^-6
2. 1.41 x 10^-10 mol² dm^-6
3. 2.0 x 10^-10 mol² dm^-6
4. 4.0 x 10^-20 mol² dm^-6

A

Q.16: An excess of silver nitrate is added to the aqueous barium chloride and the precipitate is removed by filtration. What are the main ions in the filtrate??

1. Ag⁺ and NO^–₃ only
2. NO^–₃ and Ba⁺² only
3. Ag⁺ and NO^–₃ and Ba⁺² only
4. Cl^– and NO^–₃ and Ba⁺² only

C

Q.17: The pH of 10^-4 mole dm^-3of HCl?

1. 2
2. 4
3. 3
4. 5

B

Q.18: The most suitable temperature for preparing ammonia gas is?

1. 250°C
2. 450°C
3. 350°C
4. 550°C

B

Q.19: The K_w of water at 25°C is given by?

1. 10^-7
2. 10^-10
3. 10^-12
4. 10^-14

D

Q.20: When HCl gas is passed through the saturated solution of rock salt, the solubility of NaCl?

1. Increases
2. May increases or decreases
3. Decreases
4. None of these

C

Q.21: For what value of K_c almost forward reaction is complete??

1. K_c = 10^-30
2. K_c = 1
3. K_c = 10³⁰
4. K_c = 0

C

Q.22: In which of the following Equilibria will K_c and K_p have not the same value??

1. 2HI ⇌ H₂ + I₂
2. 2SO₂ + O₂ ⇌ 2SO₃
3. N₂ + O₂ ⇌ 2NO
4. All of these

B

Q.23: If the temperature is increased of the following reaction, then will go in
N₂ + 3H₂ ⇌ 2NH₃ ∆H = -Ve?

1. Forward direction
2. Remain constant
3. Reverse direction
4. Cannot be predicted

C

Q.24: The pH of an aqueous solution is 3.0 at 25°C. The hydrogen ion concentration in the solution would be?

1. 0.001
2. 0.01
3. 0.0001
4. 10^-5

A

Q.25: Which one is very weak acid??

1. HF
2. H₂CO₃
3. HCl
4. H₂O

D

Q.26: Which one increases by common ion effect except??

1. Crystallization
2. Solubility
3. Association of ions
4. All of these

B

Q.27: A basic buffer solution can be prepared by mixing?

1. Strong acid and it is a salt with a weak base
2. Strong base and it is a salt with weak acid
3. Weak base and it is a salt with a strong acid
4. Weak acid and it is a salt with strong base

C

Q.28: Which one is the best buffer those have?

1. pH = pK_a
2. pH > pK_a
3. pOH < pK_b
4. pK_a = 0

A

Q.29: The pH of an ideal buffer is?

1. 10
2. 7
3. Less than 7
4. 0

B

Q.30: If the ionic product is equal to K_sp then the solution is?

1. Unsaturated
2. Ideal
3. Supersaturated
4. Saturated

D