Three moles of PCl3 three moles of PCl3, and two moles of Cl, are

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 Multiple Choice QuestionsMultiple Choice Questions

311.

The pH of 10-8 M HCl solution is:

  • 8

  • more than 8

  • between 6 and 7

  • slightly more than 7


312.

Hydroxyl ion concentration of 10-2 M HCl is

  • 1 × 101 mol dm-3

  • 1 × 10-12 mol dm-3

  • 1 × 10-1 mol dm-3

  • 1 × 10-14 mol dm-3


313.

A ligand can also be regarded as

  • Lewis acid

  • Bronsted base

  • Lewis base

  • Bronsted acid


314.

Which one of the following salts on being dissolved in water gives pH > 7 at 25°C?

  • KCN

  • KNO3

  • NH4Cl

  • NH4CN


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315.

Three moles of PCl3 three moles of PCl3, and two moles of Cl, 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


D.

4.5

PCl5              PCl3 +       Cl23mol                  3mol         2 mol initally(3-x)                (3+x)        (2+x)mol initally  3-x=1.5         x=1.5 NumberofmolesofPCl3 = 3+ x                                              = 3+1.5 = 4.5


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316.

For the reaction 2HI (g) H2(g) + I2(g)-Q kJ, the equilibrium constant depends upon

  • temperature

  • pressure

  • catalyst

  • volume


317.

N2 + 3H2 2NH3 + heat.What is the effect of the increase of temperature on the equilibrium of the reaction? 

  • Equilibrium is shifted to the left

  • Equtlibriumis shifted to the right

  • Equilibrium is unaltered

  • Reaction rate does not change


318.

30 cc of M3, 20 cc of M2 HNO3 and 40 cc of M4 NaOH solutions are mixed and the volume was made up to 1 dm3. The pH of the resulting solution is

  • 8

  • 2

  • 1

  • 3


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319.

10-6 M NaOH is diluted 100 times. The pH of the diluted base is

  • between 7 and 8

  • between 5 and 6

  • between 6 and 7

  • between 10 and 11


320.

2HI (g)  H2 (g) + 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, the equilibrium constant will be

  • 6.4

  • 0.8

  • 3.2

  • 1.6


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