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11th Standard Chemistry Model Question Paper 2019 K Sudhakar Jan-27 , 2019

+1 FIRST REVISION TEST

11th Standard Chemistry Model Question Paper 2019

+1 FIRST REVISION TEST

11th Standard

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Chemistry

Time : 02:30:00 Hrs
Total Marks : 70

    PART-A


    15 x 1 = 15

  1. 7.5 g of a gas occupies a volume of 5.6 litres at 0° C and 1 atm pressure. The gas is ________.

    (a)

    NO

    (b)

    N2O

    (c)

    CO

    (d)

    CO2

  2. Which of the following provides the experimental justification of magnetic quantum number?

    (a)

    Zeeman effect

    (b)

    Stark effect

    (c)

    Uncertainty principle

    (d)

    Quantum condition

  3. Which one of the following is true about metallic character when we move from left to right in a period and top to bottom in a group?

    (a)

    Decreases in a period and increases along the group

    (b)

    Increases in a period and decreases in a group

    (c)

    Increases both in the period and the group

    (d)

    Decreases both in the period and in the group

  4. Which pair are not hydrogen isotopes?

    (a)

    Ortho and para hydrogen

    (b)

    Protium and deuterium

    (c)

    Deuterium and tritium

    (d)

    Tritium and protium

  5. Which of the following has the highest tendency to give the reaction \(M_{g}^{+}\xrightarrow[Medium]{Aqueous}M_{aq}^{+}\)

    (a)

    Na

    (b)

    Li

    (c)

    Rb

    (d)

    K

  6. Identify the correct mathematical expression of Graham's law of diffusion __________

    (a)

    \(\frac { { r }_{ 2 } }{ { r }_{ 1 } } =\sqrt { \frac { { M }_{ 2 } }{ { M }_{ 1 } } } \)

    (b)

    \({ r }_{ 1 }r_{ 2 }=\sqrt { \frac { { M }_{ 2 } }{ { M }_{ 1 } } } \)

    (c)

    \(\frac { { r }_{ 1 } }{ { r }_{ 2 } } =\sqrt { \frac { { M }_{ 2 } }{ { M }_{ 1 } } } \)

    (d)

    \(\frac { { r }_{ 1 } }{ { r }_{ 2 } } ={ \left[ \frac { { M }_{ 2 } }{ { M }_{ 1 } } \right] }^{ 2 }\)

  7. If one mole of ammonia and one mole of hydrogen chloride are mixed in a closed container to form ammonium chloride gas, then _____________

    (a)

    ΔH > ΔU

    (b)

    ΔH - ΔU = 0

    (c)

    ΔH + ΔU = 0

    (d)

    ΔH < ΔU

  8. For the homogeneous gas reaction at 600K \(4NH_{ 3\left( g \right) }+5{ O }_{ 2\left( g \right) }\rightleftharpoons 4NO_{ \left( g \right) }+6{ H }_{ 2 }{ O }_{ \left( g \right) }\) The unit of equilibrium constant K" is

    (a)

    (mol dm-3)-1

    (b)

    (mol dm-3)

    (c)

    (mol dm-3)10

    (d)

    (mol dm-3)9

  9. Normality of 1.25M sulphuric acid is ___________

    (a)

    1.25 N

    (b)

    3.75 N

    (c)

    2.5 N

    (d)

    2.25 N

  10. During change of \({ O }_{ 2 }\) to \({ O }_{ 2 }^{ - }\) ion, the electron adds on which one of the following orbitals?

    (a)

    \(\pi\) orbitals

    (b)

    \(\sigma -\)orbitals

    (c)

    \(\pi^*\) orbitals

    (d)

    \(\sigma ^*\)orbitals

  11. The IUPAC name of the Compound is _____________
     

    (a)

    2,3 - Diemethylheptane

    (b)

    3- Methyl -4- ethyloctane

    (c)

    5-ethyl -6-methyloctane

    (d)

    4-Ethyl -3 - methyloctane

  12. The most stable carbocation is ____________

    (a)

    \(C{ H }_{ 3 }-\overset { + }{ C } { H }_{ 2 }\)

    (b)

    \(C{ H }_{ 3 }-\overset { + }{ C } H-C{ H }_{ 3 }\)

    (c)

    \(C{ H }_{ 2 }=CH-\overset { + }{ C } { H }_{ 2 }\)

    (d)

    \(\overset { + }{ C } { H }_{ 3 }\)

  13. In which of the following molecules, all atoms are co-planar ___________

    (a)

    (b)

    (c)

    (d)

    both (a) and (b)

  14. Ozone depletion will cause ___________.

    (a)

    forest fires

    (b)

    eutrophication

    (c)

    bio magnification

    (d)

    global warming

  15. Cause of eutrophication is ____________

    (a)

    Increase of oxygen in water bodies

    (b)

    Increase in number of aquatic organisms

    (c)

    Nutrient enrichment of water bodies

    (d)

    All ofthese

    16. PART -B


    6 x 2 = 16

  16. Calculate the equivalent masses of the following - Oxalic acid H2C2O4

  17. Magnesium loses electrons successively to form Mg+, Mg2+ and Mg3+ ions. Which step will have the highest ionisation energy and why?

  18. Lithium iodide is covalent. Explain why?

  19. Define the calorific value of food. What is the unit of calorific value?

  20. What are the non-aqueous solution ? Give example

  21. Give a brief description of the principles of
    Fractional distillation

  22. Which of the following ions is more stable ? Use resonance to explain your answer.

  23. Identify A, Band C from the following equation 

  24. What is green chemistry ?

    25. PART -C


    6 x 3 = 18

  25. Calculate the uncertainty in position of an electron, if Δv = 0.1% and \(\upsilon \) = 2.2 x 106 ms-1.

  26. Mention any two biological effects of D2O.

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

  28. Give the systematic names for the following
    Milk of magnesia

  29. Which of the following gases would you expect to deviate from ideal behaviour under conditions of low temperature F2, Cl2 or Br2? Explain.

  30. For the reaction
    SrCO3 (s) ⇌ SrO (s) + CO2(g),
    the value of equilibrium constant KP = 2.2 x 10–4 at 1002 K. Calculate KC for the reaction.

  31. What happens when the' concentration of H2 and I2 are increased in the reaction \({ H }_{ 2 }+{ I }_{ 2 }\rightleftharpoons 2HI?\)

  32. 0.40 g of an iodo-substituted organic compound gave 0.235 g of AgI by carius method. Calculate the percentage of iodine in the compound. (Ag = 108, I = 127)

  33. Carry over the following reaction mechanisms.
    (i) Bromination of alkene
    (ii) Addition of HCN to CH3CHO
    (iii) Formation of alkyl bromide with benzoyl peroxide as radical initiator.

    34. PART -D


    5 x 5 = 25

  34. A Compound on analysis gave Na = 14.31% S = 9.97% H = 6.22% and 0 = 69.5%.
    Calculate the molecular formula of the compound if all the hydrogen in the compound is present in combination with oxygen as a water of crystallization. (molecular mass of the compound is 322).

  35. The Li2+ ion is a hydrogen like ion that can be described by the Bohr model. Calculate the Bohr radius of the third orbit and calculate the energy of an electron in 4th orbit.

  36. List out and compare the chemical properties of metals and non-metals.

  37. Define hydrogen bond and its types.

  38. 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).

  39. Consider the following reaction
    Fe3+(aq) + SCN–(aq) ⇌ [Fe(SCN)]2+(aq)
    A solution is made with initial Fe3+, SCN- concentration of 1 x 10-3 M and 8 x 10-4 M respectively. At equilibrium [Fe(SCN)]2+ concentration is 2 x 10-4 M. Calculate the value of equilibrium constant.

  40. What is the molarity of the solutions prepared by diluting 25.0 mL of 0.312M MgCl2 solution to each of the following volumes (a) 40 mL
    (b) 100mL
    (c) 350mL?

  41. How is nitrogen estimated by Dumas method?

  42. Predict the product:
    (i) Chloroform + O2 ⟶?
    (ii) CCl4 + H2O ⟶?
    (iv) 
    (iv) \({ CH }_{ 3 }-CH{ Cl }_{ 2 }+KOH\overset { { C }_{ 2 }{ H }_{ 5 }{ OH }_{ 3 } }{ \longrightarrow } \)?
    (v) Ethylene glycol + 2PCI5 ⟶?

  43. How is acid rain formed ? Explain its effect

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