JEE Questions for Chemistry Equilibrium Quiz 10 - MCQExams.com

The concentration of CO2 which will be in equilibrium with 2.5 × 10–2 mol L–1 of CO at 100ºC for the reaction
  • 0.5 × 10–2 mol L–1
  • 12.5 × 10–2 mol L–1
  • 2 × 10–2 mol L–1
  • None of these is correct

Chemistry-Equilibrium-3835.png
  • 50
  • 0.02
  • 250
  • 31.25
One mole of N2 and 3 moles of H2 are mixed in a litre flask. If 50% N2 is converted into ammonia by the reaction,
Chemistry-Equilibrium-3836.png
  • 1.5
  • 3.0
  • 4.5
  • 6.0

Chemistry-Equilibrium-3838.png
  • 16.0 atm
  • 0.25 atm
  • 1 atm
  • 0.75 atm
The equilibrium constants for the reaction at 1000 K are:
Chemistry-Equilibrium-3840.png
  • 0.13
  • 7.69
  • 0.0169
  • 59.3
1 mole of hydrogen and 2 moles of iodine are taken initially in a 2 litre vessel. The number of moles of hydrogen at equilibrium is 0.2. Then the number of moles of iodine and hydrogen iodide at equilibrium are
  • 1.2, 1.6
  • 1.8, 1.0
  • 0.4, 2.4
  • 0.8, 2.0

Chemistry-Equilibrium-3843.png
  • 3 × 10–1 mol L–1
  • 3 × 10–3 mol L–1
  • 3 × 103 mol L–1
  • 3.3 × 102 mol L–1

Chemistry-Equilibrium-3845.png
  • 20000 R
  • 0.02 R
  • 5 × 10–5 R

  • Chemistry-Equilibrium-3846.png

Chemistry-Equilibrium-3848.png
  • 2.4 × 10–3
  • 4 × 10–6
  • 4 × 10–6(RT)2
  • 16 × 10–2

Chemistry-Equilibrium-3850.png

  • Chemistry-Equilibrium-3851.png
  • 2)
    Chemistry-Equilibrium-3852.png

  • Chemistry-Equilibrium-3853.png

  • Chemistry-Equilibrium-3854.png

Chemistry-Equilibrium-3856.png
  • 2.3 × 10–4
  • 3.2 × 10–6
  • 2.3 × 104
  • 3.2 × 106
The vapour density of N2O4 at a certain temperature is 30. What is the percentage dissociation of N2O4 at this temperature?
  • 53.3%
  • 10.6.6%
  • 26.7%
  • None
One mole of N2O4 (g) at 300 K is kept in a closed container under one atmosphere. It is heated to 600 K when 20% by mass of N2O4 (g) decomposes to NO2 (g). The resultant pressure is
  • 1.2 atm
  • 2.4 atm
  • 2.0 atm
  • 1.0 atm

Chemistry-Equilibrium-3860.png
  • Catalyst
  • Pressure
  • Volume
  • Temperature
The change in pressure will not affect the equilibrium constant for

  • Chemistry-Equilibrium-3861.png
  • 2)
    Chemistry-Equilibrium-3862.png

  • Chemistry-Equilibrium-3863.png
  • all the above three reactions
Which of the following oxides of nitrogen will be the most stable one?

  • Chemistry-Equilibrium-3864.png
  • 2)
    Chemistry-Equilibrium-3865.png

  • Chemistry-Equilibrium-3866.png

  • Chemistry-Equilibrium-3867.png

Chemistry-Equilibrium-3868.png
  • If the amount of C(s) is increased, less water would be formed
  • If the amount of C(s) is increased, more CO and H2 would be formed
  • If the pressure on the system is increased by halving the volume, more water would be formed
  • If the pressure on the system is increased by halving the volume, more CO and H2 would be formed.

Chemistry-Equilibrium-3870.png
  • 0.0766 atm
  • 0.0582 atm
  • 0.0388 atm
  • 0.0194 atm
On decomposition of NH4HS, the following equilibrium is established:
Chemistry-Equilibrium-3872.png
  • P atm
  • P2 atm2
  • P2/4 atm2
  • 2 P atm
Formaldehyde polymerizes to form glucose according to the reaction
Chemistry-Equilibrium-3874.png
  • 1.6 ×10–2 M
  • 1.6 ×10–4 M
  • 1.6 ×10–6 M
  • 1.6 ×10–8 M
The correct expression for Ostwald’s dilution law is

  • Chemistry-Equilibrium-3876.png
  • 2)
    Chemistry-Equilibrium-3877.png

  • Chemistry-Equilibrium-3878.png

  • Chemistry-Equilibrium-3879.png
For a weak base, the concentration of OH- at concentration C of base would be (dissociation constant = Kb)

  • Chemistry-Equilibrium-3881.png
  • 2)
    Chemistry-Equilibrium-3882.png

  • Chemistry-Equilibrium-3883.png

  • Chemistry-Equilibrium-3884.png
Which one of the following is dibasic acid ?
  • H3PO4
  • H3PO3
  • H3BO3
  • H3ASO4
Which of the following is a base according to Lowry-Bronsted concept?
  • I–
  • H3O+
  • HCl

  • Chemistry-Equilibrium-3886.png

Chemistry-Equilibrium-3887.png

  • Chemistry-Equilibrium-3888.png
  • NH3
  • N2H4
  • NH2OH
Conjugate base of Hydrazoic acid is

  • Chemistry-Equilibrium-3890.png
  • 2)
    Chemistry-Equilibrium-3891.png

  • Chemistry-Equilibrium-3892.png

  • Chemistry-Equilibrium-3893.png
According to Bronsted concept, the acids in the following reaction
Chemistry-Equilibrium-3895.png

  • Chemistry-Equilibrium-3896.png
  • 2)
    Chemistry-Equilibrium-3897.png

  • Chemistry-Equilibrium-3898.png

  • Chemistry-Equilibrium-3899.png

Chemistry-Equilibrium-3901.png
  • weak conjugate base
  • strong conjugate base
  • weak conjugate acid
  • strong conjugate acid
According to Bronsted Lowry concept, the relative strengths of the bases CH3COOH–, OH– and Cl– are in the order :
  • OH– > CH3COO– > Cl–
  • Cl– > OH– > CH3COO–
  • CH3COO– > OH– > Cl–
  • OH– > Cl– > CH3COO–
Which one of the following solutions contains the highest concentration of hydronium ion?
  • 0.1 M HBr
  • 0.1 M HCl
  • 0.1 MHI
  • 0.1 M HF
Which of the following is the weakest?

  • Chemistry-Equilibrium-3902.png
  • 2)
    Chemistry-Equilibrium-3903.png

  • Chemistry-Equilibrium-3904.png

  • Chemistry-Equilibrium-3905.png
Which of the following is not as Lewis base?
  • CN−
  • ROH
  • NH3
  • AlCl3
Which of the following is Lewis acid?
  • H2O
  • SnCl4
  • C2H5OH
  • Cl–
EDTA is a/an
  • Arrhenius acid
  • Bronsted base
  • Lewis base
  • All of the above
The pH range for phenolphthalein is
  • 3.2 - 4.5
  • 4.5 - 6.5
  • 5.5 - 7.4
  • 8.0 - 10.0
Three solutions A,B and C are prepared by adding NaCl, NaOH and HCl acid respectively. Then ionic product of water will
  • increase in A, decrease in B and C
  • increase in B, decrease in A and C
  • increase in C, decrease in A And B
  • remain the same in all the three
On adding a few drops of H2SO4 to water
  • ionic product will increase
  • ionic product will decrease
  • [OH− ] will increase
  • [OH− ] will decreases
The pH of a solution is equal to
  • log [H+]
  • 2)
    Chemistry-Equilibrium-3906.png

  • Chemistry-Equilibrium-3907.png
  • −log [H+]
pH of a 1000 cc solution is 2. It will not change if
  • 100 cc of water is added to it
  • 100 cc of 0.1 M HCl is added to it
  • 100 cc of N/100 HCl is added to it
  • 1 cc of 0.1 M HCl is added to it
The pH value of 10–3 M aqueous solution of NaCl is
  • 7
  • 3
  • 11
  • 14
Which of the following would be an acidic solution?
  • Solution having hydrogen ion concentration of 10–7 M
  • Solution having hydrogen ion concentration of 10–13 M
  • Solution having hydrogen ion concentration of 10–2 M
  • Solution having hydrogen ion concentration of 10–12 M
The tears coming out of a person’s eye have a pH of
  • 7.0
  • 7.4
  • 4.6
  • 6.4
The sum of pH and pOH in aqueous solution at 250 C is equal to
  • 7
  • 0
  • 1
  • Kw
pOH of water is 7.0 at 298 K. If water is heated to 350 K, which of the following would be true?
  • pOH will decrease
  • pOH will increase
  • pOH will remain seven
  • Concentration Of H+ ions will increase but that of OH- will decrease
The pKa of a weak acid is equal to

  • Chemistry-Equilibrium-3910.png
  • 2)
    Chemistry-Equilibrium-3911.png

  • Chemistry-Equilibrium-3912.png

  • Chemistry-Equilibrium-3913.png
The pKa of an acid whose ionisation constant, Ka = 1 × 10–10 is
  • 10
  • 4
  • – 10
  • – 4
When HCl gas is passed through a saturated solution of common salt, pure NaCl is precipitated because
  • the impurities dissolve in HCl
  • HCl is highly soluble in water
  • The ionic product of [Na+] [Cl−] exceeds the solublility product of NaCl
  • The solubility product of NaCl is lowered by Cl− from aqueous HCl
If the solubility of Ag2CrO4 is S mole/litre. Its solubility product is
  • S2
  • S3
  • 4S3
  • 2S3
If the solubility of lithium sodium hexafluoroaluminate, Li3Na3 (AlF6)2 is ‘a’ mole/litre, the solubility product is equal to
  • a8
  • 12a3
  • 18a3
  • 2916 a8
In which of the following solvents will AgBr have highest solubility ?
  • 10–3 M NaBr
  • 10–3 M NH4OH
  • Pure water
  • 10–3 M HBr
0:0:1


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