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Term II Model Question Paper

12th Standard

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Chemistry

Time : 02:30:00 Hrs
Total Marks : 70
    15 x 1 = 15
  1. Roasting of sulphide ore gives the gas (A).(A) is a colourless gas. Aqueous solution of (A) is acidic. The gas (A) is______.

    (a)

    CO2

    (b)

    SO3

    (c)

    SO2

    (d)

    H2S

  2. Cupellation is a process used for the refining of________.

    (a)

    Silver

    (b)

    Lead

    (c)

    Copper

    (d)

    iron

  3. The basic structural unit of silicates is _______.

    (a)

    \(\left( SiO_{ 3 } \right) ^{ 2- }\)

    (b)

    \(\left( SiO_{ 4 } \right) ^{ 2- }\)

    (c)

    \(\left( Sio \right) ^{ - }\)

    (d)

    \(\left( SiO_{ 4 } \right) ^{ 4- }\)

  4. Most easily liquefiable gas is _______.

    (a)

    Ar

    (b)

    Ne

    (c)

    He

    (d)

    Kr

  5. Which of the following oxidation states is most common among the lanthanoids?

    (a)

    +4

    (b)

    +2

    (c)

    +5

    (d)

    +3

  6. The sum of primary valence and secondary valence of the metal M in the complex [M(en)2(Ox)]Cl is________.

    (a)

    3

    (b)

    6

    (c)

    -3

    (d)

    9

  7. Which of the following is paramagnetic in nature?

    (a)

    [Zn(NH3)4]2+

    (b)

    [Co(NH3)6]3+

    (c)

    [Ni(H2O)6]2+

    (d)

    [Ni(CN)4]2-

  8. The ratio of close packed atoms to tetrahedral hole in cubic packing is ________.

    (a)

    1:1

    (b)

    1:2

    (c)

    2:1

    (d)

    1:4

  9. The crystal with a metal deficiency defect is ________.

    (a)

    NaCl

    (b)

    FeO

    (c)

    ZnO

    (d)

    KCl

  10. A zero order reaction X ⟶ Product, with an initial concentration 0.02M has a half life of 10 min. if one starts with concentration 0.04M, then the half life is

    (a)

    10 s

    (b)

    5 min

    (c)

    20 min

    (d)

    cannot be predicted using the given information

  11. What is the pH of the resulting solution when equal volumes of 0.1M NaOH and 0.01M HCl are mixed?

    (a)

    2.0

    (b)

    3

    (c)

    7.0

    (d)

    12.65

  12. Among the following cells
    I) Leclanche cell
    II) Nickel – Cadmium cell
    III) Lead storage battery
    IV) Mercury cell
    Primary cells are ____.

    (a)

    I and IV

    (b)

    I and III

    (c)

    III and IV

    (d)

    II and III

  13. Fog is colloidal solution of _______.

    (a)

    solid in gas

    (b)

    gas in gas

    (c)

    liquid in gas

    (d)

    gas in liquid

  14. Adsorption of a gas on solid metal surface is spontaneous and exothermic, then ______.

    (a)

    ΔH increases

    (b)

    ΔS increases

    (c)

    ΔG increases

    (d)

    ΔS decreases

  15. In the reaction Ethanol \(\overset { { PCl }_{ 5 } }{ \longrightarrow } X\overset { alc.KOH }{ \longrightarrow } Y\overset { { H }_{ 2 }{ SO }_{ 4 }/{ H }_{ 2 }O }{ \underset { 298k }{ \longrightarrow } } Z.\) The ‘Z’ is ______.

    (a)

    ethane

    (b)

    ethoxyethane

    (c)

    ethylbisulphite

    (d)

    ethanol

  16. 6 x 2 = 12
  17. Give the uses of Borax

  18. Give the uses of helium.

  19. [Ti(H2O)6]3+ is coloured, while [Sc(H2O)6]3+ is colourless- explain.

  20. Distinguish between hexagonal close packing and cubic close packing.

  21. Define solubility product.

  22. State Faraday’s Laws of electrolysis

  23. 6 x 3 = 18
  24. Give the uses of zinc.

  25. Give the uses of argon.

  26. Give the difference between double salts and coordination compounds.

  27. Define pH.

  28. Why is AC current used instead of DC in measuring the electrolytic conductance?

  29. Describe some feature of catalysis by Zeolites.

  30. 5 x 5 = 25
  31. Give the limitations of Ellingham diagram.

  32. Complete the following reactions.
    \(1. \mathrm{NaCl}+\mathrm{MnO}_{2}+\mathrm{4H}_{2} \mathrm{SO}_{4} \longrightarrow \)
    \(2. \mathrm{NaNO}_{2}+\mathrm{HCl} \longrightarrow \)
    \(3.\mathrm{P}_{4}+\mathrm{3NaOH}+\mathrm{3H}_{2} \mathrm{O} \longrightarrow \)
    \(4. \mathrm{AgNO}_{3}+\mathrm{PH}_{3} \longrightarrow \)
    \(5. \mathrm{Mg}+\mathrm{10HNO}_{3} \longrightarrow \)
    \(6. \mathrm{KClO}_{3} \stackrel{\Delta}{\longrightarrow} \)
    \(7. \mathrm{Cu}+Con. \ Hot \ \mathrm{H}_{2} \mathrm{SO}_{4} \longrightarrow\)
    \(8. \mathrm{Sb}+\mathrm{Cl}_2 \longrightarrow \)
    \(9. \mathrm{HBr}+\mathrm{H}_2 \mathrm{SO}_4 \longrightarrow \)
    \(10. \mathrm{XeF}_6+\mathrm{H}_2 \mathrm{O} \longrightarrow \)
    \(11. \mathrm{XeO}_6{ }^{4-}+\mathrm{Mn}^{2+}+\mathrm{H}^{+} \longrightarrow \)
    \(12. \mathrm{XeOF}_4+\mathrm{SiO}_2 \longrightarrow \)
    \(13. \mathrm{Xe}+\mathrm{F}_2 \frac{\mathrm{Ni} / 200 \mathrm{~atm}}{400^{\circ} \mathrm{C}}\)
    .

  33. What is crystal field splitting energy?

  34. Write a note on sacrificial protection.

  35. What is the difference between homogenous and hetrogenous catalysis?

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