JEE Questions for Chemistry Equilibrium Quiz 1 - MCQExams.com

On adding ammonia to water,
  • Ionic product will increase
  • Ionic product will decrease

  • Chemistry-Equilibrium-4120.png

  • Chemistry-Equilibrium-4121.png
Which of following base is weakest

  • Chemistry-Equilibrium-4256.png
  • 2)
    Chemistry-Equilibrium-4257.png

  • Chemistry-Equilibrium-4258.png

  • Chemistry-Equilibrium-4259.png
In the reaction H2 (g) + Cl2 (g) ⇌ 2HCl (g)
  • KP ≠ KC
  • KP = KC
  • KP > KC
  • KP < KC
Which of the following has highest pH ?

  • Chemistry-Equilibrium-3508.png
  • 2)
    Chemistry-Equilibrium-3509.png

  • Chemistry-Equilibrium-3510.png

  • Chemistry-Equilibrium-3511.png
Which is the best choice for weak base-strong acid titration?
  • Methyl red
  • Litmus
  • Phenol red
  • Phenolphthalein
The pH of 10- 4 M KOH solution will be
  • 4
  • 11
  • 10.5
  • 10
On doubling P and V with constant temperature, the equilibrium constant will
  • remain constant
  • become double
  • become one - forth
  • None of the above
What is the pH of 10-2 M H2SO4 ?
  • 1.600
  • 2
  • 10-2
  • 1.6990
2HI (g) ⇌ H2 (g) + I2 (g) - QkJ
For the above reaction, equilibrium constant depends upon
  • temperature
  • pressure
  • catalyst
  • volume

Chemistry-Equilibrium-3467.png

  • Chemistry-Equilibrium-3468.png
  • K2K3/K1

  • Chemistry-Equilibrium-3469.png

  • Chemistry-Equilibrium-3470.png

Chemistry-Equilibrium-3471.png

  • Chemistry-Equilibrium-3472.png
  • 2)
    Chemistry-Equilibrium-3473.png
  • K
  • K2
The equilibrium constant of the following are :
Chemistry-Equilibrium-3474.png

  • Chemistry-Equilibrium-3475.png
  • K2K3/K1

  • Chemistry-Equilibrium-3476.png

  • Chemistry-Equilibrium-3477.png
KP and KC are related as
  • KP = KC (RT)∆n
  • KC = KP (RT)∆n
  • KP + KC = (RT)∆n
  • KC = KP
  • KC . KP = (RT)∆n
In the synthesis of ammonia
N2 (g) + 3H2 ⇌ 2NH3 (g)
When 100 mL of N2 has reacted, the volume of H2 which has also and ammonia produced are
  • 300 mL H2 and 200 mL NH3
  • 300 mL H2 and 300 mL NH3
  • 100 mL H2 and 100 mL NH3
  • 100 mL H2 and 200 mL NH3
A quantity of PCl5 was heated in 10 dm3 vessel 250oC
PCl5 (g) ⇌ PCl3 (g) + Cl2 (g)
At equilibrium the vessel contains 0.1 mole of PCl5 and 0.2 mole of Cl2. The equilibrium constant of the reaction is
  • 0.05
  • 0.02
  • 0.025
  • 0.04
For the reaction
2NO2 (g) + 1/2 O2 ⇌ N2O5(g)
if the equilibrium constant KP then the equilibrium constant for the reaction
2N2O5(g) ⇌ 2N2O4 + O2 (g)
would be
  • KP2
  • 2/KP
  • 1/KP2
  • 2kP
A 20 litre container at 400 K contains CO2(g) at pressure 0.4 atm and an excess of SrO (neglect the volume of solid SrO). The volume of the container is now decreased by moving the movable piston fitted in the container. The maximum volume of the container, when pressure of CO2 attains its maximum value, will be :-
Chemistry-Equilibrium-3479.png
  • 10 litre
  • 4 litre
  • 2 litre
  • 5 litre

Chemistry-Equilibrium-3480.png
  • K1 > K2 > K3
  • K1 < K2 < K3
  • K1 > K3 > K2
  • K1 < K3 < K2
Consider the following gaseous equilibrium with equilibrium constants K1 and K2, respectively.
SO2 (g) + 1/2 O2 ⇌ SO3 (g)
2SO3 (g) ⇌ 2SO2 (g) + O2 (g)
The equilibrium constants are related as
  • 2K1 = K22
  • K12 = 1/K2
  • K22 = 1/K1
  • K2 = 2/K12
Final pressure is higher than initial pressure of a container filled with an ideal gas at constant temperature. What will be the value of equilibrium constant?
  • K = 1.0
  • K = 10.0
  • K > 1.0
  • K < 1.0

Chemistry-Equilibrium-3481.png
  • 10 litre
  • 4 litre
  • 2 litre
  • 5 litre
A reversible chemical reaction is having two reactants in equilibrium. If the concentration of the reactants are doubled, then the equilibrium constant will
  • be doubled
  • become one-fourth
  • be halved
  • remain the same
5 moles of SO2 and 5 moles of O2 are allowed to react. At equilibrium, it was found that 60% of SO2 is used up. If the total pressure of the equilibrium mixture is 1 atm, the partial pressure of O2 is
  • 0.82 atm
  • 0.52 atm
  • 0.21atm
  • 0.41 atm
2HI (g) ⇌ H2 + I2 (g)
The equilibrium constant of the above reaction is 6.4 at 300 K. If 0.25 mole each of H2 and I2 are added to the system at same temperature, then the equilibrium constant will be
  • 6.4
  • 0.8
  • 3.2
  • 1.6
For PCl5 ⇌ PCl3 + CL2, initial concentration of each reactant and product is 1 M. if Keq = 0.41 then
  • more PCl3 will form
  • more Cl2 will form
  • more PCl5 will form
  • no change
Which of the following is not a physical equilibrium ?
  • Ice ⇌ water
  • I2 (s) ⇌ I2 (g)
  • S (l) ⇌ S (g)
  • 3O2 ⇌ 2O3
For an equilibrium reaction, if the value of KC >> 1, then the reaction favoured more towards
  • backward
  • forward
  • equilibrium will be obtained
  • reaction will stop
If the value of KC for an equilibrium reactions is 10-4, then the reaction is in
  • backward direction
  • forward direction
  • equilibrium
  • reaction is not possible
For a reaction at equilibrium, which of the following is correct?
  • Concentration of reactant = Concentration of product
  • Concentration of reactant is always greater than that of product
  • Rate of forward reaction =Rate of backward reaction
  • QC = K
Which of the following is a wrong statement about equilibrium state?
  • Rate of forward reaction =Rate of backward reaction
  • Equilibrium is dynamic
  • Catalysts increase the value of equilibrium constant
  • Free energy change is zero
A + B ⇌ C + D
In the above reaction, initially moles of A and B are equal. At equilibrium, moles of C are three times that of A. The equilibrium constant of the reaction will be
  • 1
  • 3
  • 4
  • 9
If for N2 + 3H2 ⇌ 2NH3, keq = 1.6 × 10-5, then the value of keq for the reaction NH3 ⇌ 1/2 N2 + 3/2 H2 will be
  • 6.25
  • 25
  • 250
  • 500
3 moles of A and 4 moles of B are mixed together and allowed to come into equilibrium according to the following reaction.
3A (g) + 4B (g) ⇌ 2C (g) + 3D (g)
When equilibrium is reached, there is 1 mole of C. The equilibrium extent of the reaction is
  • 1/4
  • 1/3
  • 1/2
  • 1
Formaldehyde polymerises to form glucose according to the reaction, 6 HCHO ⇌ C6H12O6.
The theoretically computed equilibrium constant for this reaction is found to be 6 x 1022. If 1 M solution of glucose dissociates according to the above equilibrium, the concentration of formaldehyde in the solution will be
  • 1.6 × 10-2 M
  • 1.6 × 10-4 M
  • 1.6 × 10-6 M
  • 1.6 × 10-8 M
In chemical equilibrium, the value of ∆n (number of molecules of products - number of molecules of reactants), is negative, then the relationship between KP and KC will be
  • KP - KC = 0
  • KP - KC (RT)+∆ng
  • KP - KC (RT)-∆n
  • KP = 1/KC
Three moles of PCl5, three moles of PCl3 and two moles of Cl2 are taken in a closed vessel. If at equilibrium, the vessel has 1.5 moles of PCl5, the number of moles of PCl3 present in it is
  • 5
  • 3
  • 6
  • 4.5
At 600oC, KP for the following reactions is 1 atm
X (g) ⇌ Y (g) + Z (g)
At equilibrium, 50% of X(g) is dissociated. The total pressure of the equilibrium system is p atm. What is the partial pressure (in atm) of X (g) at equilibrium?
  • 1
  • 4
  • 2
  • 0.5
Equivalent amounts of H2 and I2 are heated in a closed vessel till equilibrium is obtained. If 80% of the hydrogen can be converted to HI, the valve of KC at this temperature is
  • 64
  • 16
  • 0.25
  • 4
For the reaction H2 (g) + I2 (g) ⇌ 2 HI (g), the equilibrium constant KP changes with
  • total pressure
  • catalyst
  • the amount of HI and I2
  • temperature
A + B ⇌ C + D. If initially the concentration of both A and B are both equal but at equilibrium, concentration of D will be twice of that of A, then what will be the equilibrium constant of reaction?
  • 4/9
  • 9/4
  • 1/9
  • 4

Chemistry-Equilibrium-3483.png
  • 1.8 × 10–3
  • 3.6 × 10–3
  • 6.0 × 10–2
  • 1.3 × 10–5
In the reaction 3A + 2B → 2C, the equilibrium constant KC is given by

  • Chemistry-Equilibrium-3484.png
  • 2)
    Chemistry-Equilibrium-3485.png

  • Chemistry-Equilibrium-3486.png

  • Chemistry-Equilibrium-3487.png
N2 and H2 in 1 : 3 molar ratio are heated in a closed container having a catalyst. When the following equilibrium, N2 (g) + 3H2 (g) ⇌ 2NH3 (g) is attained, the total pressure is 10 atm and mole fraction of NH3 is 0.60. The equilibrium constant KP for dissociation of NH3 is
  • 1.333 atm-2
  • 0.75 atm2
  • 0.75 atm-2
  • 1.333 atm2
The chemical equilibrium of a reversible reaction is not influenced by
  • pressure
  • catalyst
  • concentration of the recatnts
  • temperature
15 moles of H2 and 5.2 moles of I2 are mixed and allowed to attain equilibrium at 500oC. At equilibrium, the concentration of HI is found to be 10 moles. The equilibrium constant for the formation of HI is
  • 50
  • 15
  • 100
  • 25
The rate at which a substance reacts depends on its
  • atomic weight
  • atomic number
  • molecular weight
  • active mass
For the reaction,
N2 (g) + O2 (g) ⇌ 2NO (g), the value of KC at 800°C is 0.1. When the equilibrium concentration of both the reactants is 0.5 mole, what is the value of KP at the same temperature ?
  • 0.5
  • 0.1
  • 0.01
  • 0.025
A (g) + 3B (g) ⇌ 4C (g)
Initially, concentration of A is equal to that of B. The equilibrium concentrations of A and C are equal. KC is equal to
  • 0.08
  • 0.8
  • 8
  • 80
  • 1/8
2 moles of PC15 is heated in a closed vessel of 2 L capacity. When the equilibrium is attained 40% of it has been found to be dissociated. What is the value (in mol/dm3) of KC ?
  • 0.532
  • 0.266
  • 0.133
  • 0.174
  • 0.25
For the reaction,
H2 (g) + CO2 (g) ⇌ CO (g) + H2O (g), if the initial concentration of [H2] = [CO2] and x mol/L of hydrogen is consumed at equilibrium, the correct expression of KP is

  • Chemistry-Equilibrium-3488.png
  • 2)
    Chemistry-Equilibrium-3489.png

  • Chemistry-Equilibrium-3490.png

  • Chemistry-Equilibrium-3491.png
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