11-Std 3rd Revision Test

11th Standard

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Chemistry

Time : 02:30:00 Hrs
Total Marks : 70
    15 x 1 = 15
  1. Assertion: The number of oxygen atoms in 16g of oxygen and 16g of ozone is same 
    Reason Each of the species represent 1g atom of oxygen

    (a)

    Both assertion and reason are correct and the reason is the correct explanation for an assertion

    (b)

    Both assertion and reason are correct but a reason  is not the correct explanation for assertion

    (c)

    Assertion is true but reason are false.

    (d)

    Both assertion and reason are false

  2. The total number of orbitals associated with the principal quantum number n = 3 is

    (a)

    9

    (b)

    8

    (c)

    5

    (d)

    7

  3. Which of the following statement is incorrect?

    (a)

    The ionization potential of nitrogen is greater than that of oxygen

    (b)

    The electron affinity of F is greater than that of Cl.

    (c)

    The ionization potential of Mg is greater than aluminium.

    (d)

    The electronegativity of F is greater than that of Cl.

  4. Zeolite used to soften hardness of water is hydrated

    (a)

    Sodium aluminium silicate

    (b)

    Calcium aluminium silicate

    (c)

    Zinc aluminium borate

    (d)

    Lithium aluminium hydride

  5. The suspension of slaked lime in water is known as

    (a)

    lime water

    (b)

    quick lime

    (c)

    milk of lime

    (d)

    aqueous solution of slaked lime

  6. Compressibility factor for CO2 at 400 K and 71.0 bar is 0.8697. The molar volume of CO2 under these conditions is

    (a)

    22.04 dm3

    (b)

    2.24 dm3

    (c)

    0.41 dm3

    (d)

    19.5 dm3

  7. Change in internal energy, when 4 kJ of work is done on the system and 1 kJ of heat is given out by the system is

    (a)

    +1 kJ

    (b)

    - 5 kJ

    (c)

    +3 kJ

    (d)

    - 3 kJ

  8. For the reaction \(A+3B\rightleftharpoons 2C+D\) initial mole of A is twice that of B.1f at equilibrium moles of B and C are equal, then percent of B reacted is

    (a)

    10%

    (b)

    20%

    (c)

    40%

    (d)

    60%

  9. The correct equation for the degree of an associating solute, 'n' molecules of which undergoes association in solution, is

    (a)

    \(\alpha={n(i-1)\over n-1}\)

    (b)

    \(\alpha^2={n(1-i)\over (n-1)}\)

    (c)

    \(\alpha={n(i-1)\over 1-n}\)

    (d)

    \(\alpha={n(1-i)\over n(1-i)}\)

  10. In which of the following bond angle is maximum?

    (a)

    NH3

    (b)

    PCI3

    (c)

    \({ NH }_{ 4 }^{ + }\)

    (d)

    SCl2

  11. A sample of 0.5g of an organic compound was treated according to Kjeldahl’s method. The ammonia evolved was absorbed in 50mL of 0.5M H2SO4. The remaining acid after neutralisation by ammonia consumed 80mL of 0.5 MNaOH, The percentage of nitrogen in the organic compound is.

    (a)

    14%

    (b)

    28%

    (c)

    42%

    (d)

    56%

  12. Heterolytic fission of C-Br bond results in the formation of

    (a)

    free radical

    (b)

    Carbanion

    (c)

    Carbocation

    (d)

    Carbanion and Carbocation

  13. How many stereoisomers does the molecules have? CH3CH=CHCH2CHBrCH3

    (a)

    2

    (b)

    4

    (c)

    6

    (d)

    8

  14. The order of correct bond energy of C - X bond is

    (a)

    C-CI>C-I>C-Br

    (b)

    C - CI > C - Br > C - I

    (c)

    C - I> C - CI > C - Br

    (d)

    C -I > C - Br > C - CI

  15. Bhopal Gas Tragedy is a case of _____________

    (a)

    thermal pollution

    (b)

    air pollution

    (c)

    nuclear pollution

    (d)

    land pollution

  16. 6 x 2 = 12
  17. How much volume of Carbon dioxide is produced when 25 g of calcium carbonate is heated completely under standard conditions?

  18. An atom of an element contains 35 electrons and 45 neutrons. Deduce
    (i) the number of protons
    (ii) the electronic configuration for the element
    (iii) All the four quantum numbers for the last electron

  19. State Mendeleev's periodic law.

  20. What are isobar and isochores?

  21. Consider the following equilibrium reactions
    and relate their equilibrium, constants
    i) N2 + O2 ⇌ 2NO ; K1
    ii) 2NO + O2 ⇌ 2NO2 ; K2
    iii) N2 + 2O2 ⇌ 2NO2 ; K3

  22. Identify the magnetic nature of the anion of Na2O2.

  23. Describe optical isomerism with suitable example.

  24. Draw the resonating structure of C6H5NH2 .

  25. Why chlorination of methane is not possible in dark?

  26. 6 x 3 = 18
  27. How much volume of chlorine is required to form 11.2 L of HCI at 273 K and 1 atm pressure?

  28. State the findings of modern periodic law.

  29. Do you think that heavy water can be used for drinking purposes?

  30. State Boyle's law.

  31. Define the Molar Heat of Fusion

  32. The observed depression in freezing point of water for a particular solution is 0.093o C. Calculate the concentration of the solution in molality. Given that molal depression constant for water is 1.86 KKg mol-1.

  33. Represent and explain the structures of acetaldoxime.

  34. Write a short note on the following.
    (i) Aromatisation
    (ii) Pyrolysis

  35. Even though the use of pesticides increases the crop production, they adversely affect the living organisms. Explain the function and the adverse effects of the pesticides.

  36. 5 x 5 = 25
  37. Write the steps to be followed for writing empirical formula.

  38. What is screening effect? Briefly give the basis for pauling's scale of electronegativity.

  39. Explain (i) intermolecular hydrogen bond and
    (ii) intramolecular hydrogen bond.

  40. Alkaline earth metal (A), belongs to 3rd period reacts with oxygen and nitrogen to form compound (B) and (C) respectively. It undergo metal displacement reaction with AgNO3 solution to form compound (D).

  41. A tank of oxygen has a volume of 2.5 L at a pressure of 5.0 atm. What would be the volume of oxygen at 1.01 atm?

  42. Calculate the entropy change in the system, and surroundings, and the total entropy change in the universe during a process in which 245 J of heat flow out of the system at 77°C to the surrounding at 33°C.

  43. The equilibrium constant at 298 K for a reaction is 100.
    A + B \(\rightleftharpoons \) C + D
    If the initial concentration of all the four species is 1 M, the equilibrium concentration of D (in mol lit-1) will be

  44. Consider the structures I to VII and answer the following questions (i) to (v)
    (i) CH3-CH2-CH2-CH2-OH
    (ii) \({ CH }_{ 3 }-{ CH }_{ 2 }-\underset { \overset { | }{ OH } }{ CH } -{ CH }_{ 3 }\)
    (iii) \({ CH }_{ 3 }-\overset { \underset { | }{ { CH }_{ 3 } } }{ \underset { \overset { | }{ { CH }_{ 3 } } }{ C } } -{ CH }_{ 3 }\)
    (iv) \({ CH }_{ 3 }-\underset { \overset { | }{ { CH }_{ 3 } } }{ { CH }_{ 3 } } -{ CH }_{ 2 }-OH\)
    (v) CH3 -CH2 -O-CH2 -CH3
    (vi) CH3 - O - CH2 - CH2 - CH3
    (vii) \({ CH }_{ 3 }-O-\underset { \overset { | }{ { CH }_{ 3 } } }{ { CH } } -{ CH }_{ 3 }\)
    (i) Which of the above compounds form pairs of metamers?
    (ii) Identify the pairs of compounds which are functional isomers.
    (iii) Identify the pairs of compounds that represent position isomerism.
    (iv) Identify the pairs of compounds that represent chain isomerism.
    (v) Does any of these compounds possess geometrical isomerism? If yes identify them. If no, give reason.
     

  45. Give a detailed account on the different mechanisms followed in elimination reaction.

  46. Differentiate the following
    (i) BOD and COD
    (ii) Viable and non-viable particulate pollutants

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