1st Year Chemistry Chemical Equilibrium MCQs

If you are searching for Entry Test MCQs then the 1st Year Chemistry Chemical Equilibrium MCQs are available here. This chapter is about Chemical Equilibrium. There are two types of Chemical Reactions i.e. Reversible and Irreversible reactions. Reversible Reactions are in the format of Chemical Equilibrium. For the chemical reactions, the law of Mass Action is very significant. The reactions in the equilibrium state are stated by Equilibrium constant. There are some advantages of equilibrium constants. Le-Chatelier’s principle gives some importance to Chemical Equilibrium. Applications of Chemical Equilibrium consists of the Synthesis of Ammonia and Preparation of Sulphur Trioxide. Acids and bases have their own Ionization Constants. Lowry Bronsted gave the concepts of acid and base. Some applications are Common Ion Effect and Buffer Solutions. Solubility product has some advantages in Chemical Reactions. So, you can get the important MCQs of this chapter on this page below.

1st Year Chemistry Chemical Equilibrium MCQs

KEY POINTS

 

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

• 1
• 0
  
• 2
• Less than 0

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

• 2
• 12
  
• 0
• 2.7

Question#3. Buffer solutions are used in except?

• Clinical analysis
• Nutrition
• Soil science
• Qualitative analysis

Question#4. Buffer action can be explained by except?

• Common ion effect
• Le-Chatelier’s principle
• Law of mass action
• Solubility product

Question#5. At equilibrium, the concentration of reactants and products are:

• Constant
  
• Maximum
• Different
• Equal

Question#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:

• Low temperature and high pressure
• High temperature and low pressure
• Low temperature and low pressure
• High temperature and high pressure

Question#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?

• It increases
• It remains unaffected
• It decreases
• Can’t be predicted without K_P

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

• Temperature is increased and pressure is kept constant
• Temperature is reduced and pressure is increased
• Both temperature and pressure are increased
• Both temperature and pressure are decreased

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

• pH = pK_a
• pH = pK_b
• pH > pK_a
• pH > pK_b

Question#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?

• 1.0 x 10^-5
• 0.1 x 10^-5
• 1.0 x 10^-15
• 1.0 x 10-¹⁰

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

• 9x³
• 27x⁴
  
• 3x⁴
• 9x⁴

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

• Total pressure
• The concentration of H₂ and I₂
• Catalyst
• Temperature

Question#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______.

• 0.01
• 0.001
• 0.02
• 0.002

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

• More ice is formed
• The amount of ice and water will remain the same
• More ice is melted
• Both a and b

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

• 1.41 x 10^-5 mol² dm^-6
•  1.41 x 10^-10 mol² dm^-6
• 2.0 x 10^-10 mol² dm^-6
• 4.0 x 10^-20 mol² dm^-6

Question#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?

• Ag⁺ and NO^–₃ only
• NO^–₃ and Ba⁺² only
• Ag⁺ and NO^–₃ and Ba⁺² only
• Cl^– and NO^–₃ and Ba⁺² only

Question#17. The pH of 10^-4 mole dm^-3of HCl:

• 2
• 4
  
• 3
• 5

Question#18. The most suitable temperature for preparing ammonia gas is:

• 250°C
• 450°C
• 350°C
• 550°C

Question#19. The K_w of water at 25°C is given by:

• 10^-7
• 10^-10
• 10^-12
• 10^-14

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

• Increases
• May increases or decreases
• Decreases
• None of these

Question#21. For what value of K_c almost forward reaction is complete?

• K_c = 10^-30
• K_c = 1
• K_c = 10³⁰
• K_c = 0

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

• 2HI ⇌ H₂ + I₂
• 2SO₂ + O₂ ⇌ 2SO₃
• N₂ + O₂ ⇌ 2NO
• All of these

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

• Forward direction
• Remain constant
• Reverse direction
• Cannot be predicted

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

• 0.001
  
• 0.01
• 0.0001
• 10^-5

Question#25. Which one is very weak acid?

• HF
• H₂CO₃
• HCl
• H₂O

Question#26. Which one increases by common ion effect except?

• Crystallization
• Solubility
  
• Association of ions
• All of these

Question#27. A basic buffer solution can be prepared by mixing:

• Strong acid and it is a salt with a weak base
• Strong base and it is a salt with weak acid
• Weak base and it is a salt with a strong acid
• Weak acid and it is a salt with strong base

Question#28. Which one is the best buffer those have:

• pH = pK_a
• pH > pK_a
• pOH < pK_b
• pK_a = 0

Question#29. The pH of an ideal buffer is:

• 10
• 7
• Less than 7
• 0

Question#30. If the ionic product is equal to K_sp then the solution is:

• Unsaturated
• Ideal
• Supersaturated
• Saturated