JEE Questions for Chemistry Equilibrium Quiz 2 - MCQExams.com

In which of the following equilibrium systems, is the rate of the backward reaction favoured by increase of pressure?
  • PCl5 ⇌ PCl3 + Cl2
  • 2SO2 + O2 ⇌ 2SO3
  • N2 + 3H2 ⇌ 2NH3
  • N2 + O2 ⇌ 2NO
In the lime kiln, the reaction
CaCO3 (s) → CaO (s) + CO2 (g) goes to completion because
  • of high temperature
  • CaO is more stable than CaCO3
  • CO2 escapes simultaneously
  • CaO is not dissociated
  • CO2 is gaseous product
In a reversible chemical reaction at equilibrium if the concentration of any one of the reactants is doubled, then the equilibrium constant will
  • also be doubled
  • be halved
  • remain the same
  • become one-fourth
N2 (g) + 3H2(g) ⇌ 2NH3(g)
In the reaction given above, the addition of small amount of an inert gas at constant pressure will shift the equilibrium towards which side?
  • LHS (Left Hand Side)
  • RHS (Right Hand side)
  • Neither side
  • Either side
According to Le-Chatelier's principle, the addition of temperature to the following reaction
CO2 (g) + 2H2O (g) → CH4 (g) + 2O2
will cause it to the right. This reaction is, therefore
  • exothermic
  • unimolecular
  • endothermic
  • spontaneous
N2 + 3H2 ⇌ 2NH3 + Heat. What is the effect of the increasing of temperature on the equilibrium of the reaction?
  • Equilibrium is shifted to the left
  • Equilibrium is shifted to the right
  • Equilibrium is unaltered
  • Reaction rate does not change
Formation of SO3 from SO2 and O2 is favoured by
  • increase in pressure
  • decrease in pressure
  • increase in temperature
  • decrease in temperature
What happens to the yield on application of high pressure in the Haber's synthesis of ammonia?
  • Increases
  • Decreases
  • Unaffected
  • Reaction stops
When hydrogen molecules decomposed into its atoms, which condition gives maximum yield of H-atom ?
  • High temperature and low pressure
  • Low temperature and high pressure
  • High temperature and high pressure
  • Low temperature and low pressure
Given the equilibrium system
NH4 Cl (s) ⇌ NH4+ (aq) + Cl- (aq)
(∆H = +3.5 kcal/mol)
What change will shift the equilibrium to the right?
  • Decreasing the temperature
  • Increasing the temperature
  • Dissolving NaCl crystals in the equilibrium mixture
  • Dissolving NH4NO3 crystals in the equilibrium mixture
Consider the reaction equilibrium,
2SO2 (g) + O2 (g) ⇌ 2SO3 (g); ∆Ho = - 198 kJ
On the basis of Le-Chatelier's principle, the condition favourable for the forward reaction is
  • lowering of temperature as well as pressure
  • increasing temperature as well as pressure
  • lowering the temperature and increasing the pressure
  • any value of temperature and pressure
For the chemical reaction
3X (g) + Y (g) ⇌ X3 Y (g), the amount of X3Y at equilibrium is affected by
  • temperature and pressure
  • temperature only
  • pressure only
  • temperature, pressure and catalyst
According to Le-Chatelier's principle, adding heat of a solid and liquid in equilibrium will cause the
  • amount of solid to decrease
  • amount of liquid to decrease
  • temperature to rise
  • temperature to fall
For the reaction
N2 (g) + 3H2 (g) ⇌ 2NH3 (g);
∆H = -93.6KJ mol-1, the concentration of NH3 at equilibrium can be increased by
I. lowering the temperature
II. low pressure
III. excess of N2
IV. excess of H2
The correct is/are
  • II and IV
  • Only II
  • I, III and III
  • III and IV
  • I , III and IV
In the manufacturing of ammonia by haber's process,
N2 (g) + 3H2 ⇌ 2 NH3 (g) + 92.3KJ
Which of the following condition is unfavourable ?
  • Increasing the temperature
  • Increasing the pressure
  • Reducing the temperature
  • Removing ammonia as it is formed
The gaseous reaction,
A + B ⇌ 2C + D + Q is most favoured at
  • low temperature and high pressure
  • high temperature and high pressure
  • high temperature and low pressure
  • low temperature and low pressure
For the gaseous reaction, C2H4 + H2 ⇌ C2H6; ∆H = - 130 KJ mol-1 carried in a closed vessel, the equilibrium concentration of C2H6 can definitely be increased by
  • increasing temperature and decreasing pressure
  • decreasing temperature and increasing pressure
  • increasing temperature and pressure both
  • decreasing temperature and pressure both
In a lime kiln, to get higher yield of CO2, the measure that can be taken is
  • to remove CaO
  • to add more CaCO3
  • to maintain high temperature
  • to pump out CO2
Which one of the following is the weakest acid?
  • HF
  • HCl
  • HBr
  • Hl
Strongest conjugate base is
  • ClO-
  • ClO-2
  • ClO-3
  • ClO-4
HA is a weak acid. The pH of 0.1 M HA solution is 2. What is the degree of dissociation (a) of HA ?
  • 0.5
  • 0.2
  • 0.1
  • 0.301
Which of the following is the strongest base?

  • Chemistry-Equilibrium-3493.png
  • 2)
    Chemistry-Equilibrium-3494.png

  • Chemistry-Equilibrium-3495.png

  • Chemistry-Equilibrium-3496.png
What kind of molecule AlCl3 is ?
  • Bronsted acid
  • Lewis acid
  • Lewis base
  • Bronsted base
Which is a Lewis base ?
  • B2H6
  • LiAlH4
  • AlH3
  • NH3
Which of the following acid is stronger than benzoic acid (Ka = 6.3 × 10-5) ?
  • A (Ka = 1.67 × 10-8)
  • B (PKa = 6.0)
  • C (PKa = 4.0)
  • D (Ka = 1.0 × 10-5)
For a diprotic acid, which of the following is true for 1st and 2nd ionisation constants (Ka1 and Ka2) ?
  • Ka1 = Ka2
  • Ka1 > Ka2
  • Ka2 > Ka1
  • Ka2 ≥ Ka1
A weak monobasic acid is 1% ionised in 0.1 M solution at 25oC. The percentage of ionisation in its O. 025M solution is
  • 1
  • 2
  • 3
  • 4
  • 5
Which is lewis acid?
  • BF3
  • NF3
  • Cl-
  • H2O
Which one of the following species acts as both Bronsted acid and base ?
  • H2PO2-
  • HPO32-
  • HPO42-
  • All of these
An example of a Lewis acid is
  • MgCl2
  • SnCl4
  • AlCl3
  • NaCl
Conjugate acid of S2O82- is
  • H2S2O8
  • H2SO4
  • HS2O8-
  • HSO4-
Which of the following is a Lewis base ?
  • NaOH
  • NH3
  • BCl3
  • All of these
Which one of the following is not an amphoteric substance ?
  • HNO3
  • HCO3-
  • H2O
  • NH3
The conjugate acid of NH2- is
  • N2H4
  • NH4+
  • NH2OH
  • NH3
Ostwald's dilution law is applicable for
  • weak electrolyte
  • strong electrolyte
  • both weak and strong electrolyte
  • non-electrolyte
Which of the following is a Lewis acid ?
  • AlCl3
  • Cl-
  • CO
  • C2H2
Arrange HN4+, H2O, H3O+, HF and OH- in increasing order of acidic nature
  • H3O+ < NH4+ < HF < OH- < H2O
  • NH4+ < HF < H3O+ < H2O < OH-
  • OH- < H2O < NH4+ < HF < H3O+
  • H3O+ > HF > H2O > NH4+ > OH-
If the value of an equilibrium constant for a particular reaction is 1.6 × 1012, then at equilibrium the system will contain :-
  • mostly reactants
  • mostly products
  • similar amounts of reactants and products
  • all reactants
The values of dissociation constant of bases are given below. Which is the weakest base?
  • 1.8 × 10-5
  • 4.8 × 10-10
  • 7.2 × 10-11
  • 7.07× 10-7
The species among the following, which can act as an acid and a base is
  • HSO4-
  • SO42-
  • H3O+
  • Cl-
Which molecule is an electron donor?
  • NH3
  • BF3
  • PF5
  • AsF5
Which of these is a Lewis acid ?
  • AlCl3
  • NCl3
  • HCl
  • ROR
Among BMe3, BF3, BCl3 and B2H6, which one will be the best Lewis acid ?
  • BCl3
  • BMe3
  • B2H6
  • BF3
Which of the following is not a Lewis, acid ?
  • BF3
  • AlCl3
  • SO2
  • H2O
Which is a Lewis acid ?
I2 + I- → I3-
  • I2
  • I3-
  • I-
  • None of these
Metal ions like Ag+, Cu2+ etc, act as
  • Bronsted acids
  • Bronsted bases
  • Lewis acids
  • Lewis bases
0.023 g of sodium metal is reacted with 100 cm3 of water. The pH of the resulting solution is
  • 10
  • 11
  • 9
  • 12
The pH of 10-10 M NaOH solution is nearest to
  • -4
  • -10
  • 4
  • 7
The pH of a neutral water sample is 6.5. Then, the temperature of water
  • is 25oC
  • is more than 25oC
  • is less than 25oC
  • can be more or loss than 25oC
On mixing equal volumes of two buffer solutions of pH value 3 and 5, the pH of the resultant solution will be
  • 3.3
  • 4.0
  • 4.7
  • 5.3
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