New ! Chemistry MCQ Practise Tests



  1. Home
  2. 11th Standard
  3. Chemistry
  4. 11th Standard Chemistry Revision Test Model Question Paper 2019

Updated 11th Standard Chemistry Study Materials 2022-2023 Exams

11th Standard Chemistry Revision Test Model Question Paper 2019 Feb-18 , 2019

+1 First Revision Test 2019

11th Standard Chemistry Revision Test Model Question Paper 2019

+1 First Revision Test 2019

11th Standard

    Reg.No. :
  •  
  •  
  •  
  •  
  •  
  •  

Chemistry

Time : 02:30:00 Hrs
Total Marks : 70
    15 x 1 = 15

  1. In the reaction 2AuCl3 + 3SnCl2 \(\rightarrow\) 2Au + 3SnCl4 which is an oxidising agent?

    (a)

    AuCl3

    (b)

    Au

    (c)

    SnCl2

    (d)

    Both AuCl3 and SnCl2

  2. What is the maximum numbers of electrons that can be associated with the following set of quantum numbers? n = 3, I = 1 and m =-1

    (a)

    4

    (b)

    6

    (c)

    2

    (d)

    = 10

  3. In the modern periodic table, the period indicates the value of____

    (a)

    atomic number

    (b)

    mass number

    (c)

    principal quantum number

    (d)

    azimuthal quantum number

  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 name 'Blue John' is given to which of the following compounds ?

    (a)

    CaH2

    (b)

    CaF2

    (c)

    Ca2(PO4)2

    (d)

    CaO

  6. The value of the gas constant R is ____________

    (a)

    0.082 dm3 atm.

    (b)

    0.987 cal mol-1K-1

    (c)

    8.3 J mol-1 K-1

    (d)

    8 erg mol-1 K-1

  7. ΔS is expected to be maximum for the reaction ____________

    (a)

    Ca(S)+ 1/2O2(g) ⟶ CaO(S)

    (b)

    C(S) + O2(g) ⟶ CO2(g)

    (c)

    N2(g) + O2(g) ⟶ 2NO(g)

    (d)

    CaCO3(S) ⟶ CaO(S) + CO2(g)

  8. For the reaction  \({ CH }_{ 4\left( g \right) }+2O_{ 2\left( g \right) }\rightleftharpoons { CO }_{ 2\left( g \right) }+2{ H }_{ 2 }O_{ \left( l \right) }\) \(\Delta H\) = -170.8 KJ mol-1 which of the following statement is not true?

    (a)

    At equilibrium, the concentration of CO2(g) and H20(l) are not equal

    (b)

    The equilibrium constant for the reaction is given by \({ K }_{ p }=\cfrac { \left[ { CO }_{ 2 } \right] }{ \left[ { CH }_{ 4 } \right] \left[ { O }_{ 2 } \right] } \)

    (c)

    Addition of CH4(g) or 02(g) at equilibrium will cause a shift to the right

    (d)

    The reaction is exothermic.

  9. The Henry's law constant for the solubility of Nitrogen gas in water at 350 K is 8 x 104 atm. The mole fraction of nitrogen in air is 0.5. The number of moles of Nitrogen from air dissolved in 10 moles of water at 350K and 4 atm pressure is ____________

    (a)

    4 x 10-4

    (b)

    4 x 104

    (c)

    2 x 10-2

    (d)

    2.5 x 10-4

  10. Identify the correct order of the diatomic species arranged in their increasing order of bond order.

    (a)

    \({ He }_{ 2 }^{ + }<{ O }_{ 2 }^{ - }

    (b)

    \(<{ C }_{ 2 }^{ 2- }<{ He }_{ 2 }^{ + }<{ O }_{ 2 }^{ - }

    (c)

    \(<{ O }_{ 2 }^{ - }

    (d)

    \(NO<{ { O }_{ 2 }^{ - }

  11. Lassaigne’s test for the detection of nitrogen fails in ______________

    (a)

    H2N – CO– NH.NH2.HCl

    (b)

    NH2 – NH2. HCl

    (c)

    C6H5 – NH – NH2. HCl

    (d)

    C6H5 CONH2

  12. Hyper Conjugation is also known as ___________.

    (a)

    no bond resonance

    (b)

    Baker - nathan effect

    (c)

    both (a)and (b)

    (d)

    none of these

  13. In E1, reaction, the intermediate formed is ___________

    (a)

    Carbanion

    (b)

    Carbocation

    (c)

    Carbon free radical

    (d)

    Carbene

  14. In SN1, the rate of the reaction depends on the ______________.

    (a)

    nucleophile

    (b)

    medium

    (c)

    concentration of the substrate

    (d)

    none of the above

  15. Assertion (A) : Excessive use of chlorinated pesticide causes soil and water pollution.
    Reason (R) : Such pesticides are non-biodegradable.
    i) Both (A) and R are correct and (R) is the correct explanation of (A)
    ii) Both (A) and R are correct and (R) is not the correct explanation of (A)
    iii) Both (A) and R are not correct
    iv) (A) is correct but( R) is not correct

    (a)

    Both (A) and R are correct and (R) is the correct explanation of (A)

    (b)

    Both (A) and R are correct and (R) is not the correct explanation of (A)

    (c)

    Both (A) and R are not correct

    (d)

    (A) is correct but( R) is not correct

    16. 7x 2 = 14

  16. How much volume of chlorine is required to prepare 89.6 L of HCI gas at STP?

  17. Consider the following electronic arrangements for the d5 configuration.
    (a)

    \(\upharpoonleft \downharpoonright \) \(\upharpoonleft \downharpoonright \) \(​​\upharpoonleft \)    

    (b)

    \(​​\upharpoonleft \) \(​​\upharpoonleft \) \(​​\upharpoonleft \) \(\upharpoonleft \downharpoonright \)  

    (c)

    \(​​\upharpoonleft \) \(​​\upharpoonleft \) \(​​\upharpoonleft \) \(​​\upharpoonleft \) \(​​\upharpoonleft \)

    which of these represents the ground state

  18. Account for the difference in size of Na +(95 pm) and Mg+2(65pm) both of which have the same noble gas configuration

  19. State Dalton's law of partial pressure.

  20. For a gaseous homogeneous reaction at equilibrium, number of moles of products are greater than the number of moles of reactants. Is KC is larger or smaller than KP.

  21. Why \(\sigma\) bond is stronger than \(\pi\) bond ?

  22. Explain varions types of constitutional isomerism (structural isomerism) in organic compounds

  23. Classify the following reactions in one of the reaction type studied in this unit.
    (i) \(C{ H }_{ 3 }C{ H }_{ 2 }Br+H\overset { - }{ S } \longrightarrow C{ H }_{ 3 }C{ H }_{ 2 }SH+Br\)
    (ii) \({ \left( C{ H }_{ 3 } \right) }_{ 2 }C=C{ H }_{ 2 }+HCl\longrightarrow { \left( C{ H }_{ 3 } \right) }_{ 2 }CCl-C{ H }_{ 3 }\)
    (iii) \(C{ H }_{ 3 }-C{ H }_{ 2 }Br+H\overset { - }{ O } \longrightarrow C{ H }_{ 2 }=C{ H }_{ 2 }+{ H }_{ 2 }O+Br\)
    (iv) \({ \left( { CH }_{ 3 } \right) }_{ 3 }C-C{ H }_{ 2 }OH+HB\longrightarrow { \left( C{ H }_{ 3 } \right) }_{ 2 }CBr-C{ H }_{ 2 }-C{ H }_{ 3 }+{ H }_{ 2 }O\)

  24. Which alkyl halide from the following pair is
    i) chiral
    ii) undergoes faster SN2 reaction?

    25. 7 x 3 = 21

  25. How much volume of carbon dioxide is produced when 50 g of calcium carbonate is heated completely under standard conditions ?

  26. Given the formula of the species that will be isoelectronic with the following atoms or ions
    (i) Ar
    (ii) F-
    (iii) K+
    (iv) S-2

  27. What are isotopes? Write the names of isotopes of hydrogen.

  28. When the driver of an automobile applies brake, the passengers are pushed toward the front of the car but a helium balloon is pushed toward back of the car. Upon forward acceleration the passengers are pushed toward the front of the car. Why?

  29. (a) Under what condition, the heat evolved or absorbed in a reaction is equal to its free energy change?
    (b) Calculate the entropy change for the following reversible process.
    \(H_2 O \rightleftharpoons H_2O_{I} \) Δfus H is 6 kJ mol-1

  30. 0.24 g of a gas dissolves in 1 L of water at 1.5 atm pressure. Calculate the amount of dissolved gas when the pressure is raised to 6.0 atm at constant temperature.

  31. Complete the following reactions:
    (i) \(({ CH }_{ 3 }COO)_{ 2 }pb+Na_{ 2 }S\rightarrow ?\)
    (ii) \({ Na }_{ 2 }[(Fe(CN)_{ 5 }NO]+{ Na }_{ 2 }S\rightarrow ?\)
    (iii) \(NaCNS+FeCI_{ 3 }\rightarrow ?\)
    (iv) \(Na_{ 2 }S+AgNO_{ 3 }\rightarrow ?\)
    (v) \(BaCI_{ 2 }+{ Na }_{ 2 }{ SO }_{ 4 }\rightarrow ?\)
    (vi) \({ Na }_{ 4 }[Fe(CN)_{ 6 }]+{ FeCI }_{ 3 }\rightarrow ?\)

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

  33. On the basis of chemical reactions involved, explain how do CFC’s cause depletion of ozone layer in stratosphere ?

    34. 5 x 5 = 25

    1. A compound on analysis gave the following percentage composition: C = 24.47%, H = 4.07 %, CI = 71.65%. Find out its empirical formula.

    2. Explain the following, give appropriate reasons.
      (i) Ionisation potential of N is greater than that of O.
      (ii) First ionisation potential of C-atom is greater than that of B atom, where as the reverse is true is for second ionisation potential.
      (iii) The electron affinity values of Be, Mg and noble gases are zero and those of N (0.02 eV) and P (0.80 eV) are very low.
      (iv) The formation of F-(g) from F(g) is exothermic while that of O2-(g) from O (g) is endothermic.

    1. Bond angle of water is reduced from 109.28° to 104.5°. Explain.

    2. Discuss the similarities between beryllium and aluminium.

    1. Which of following flasks has higher pressure
      (a) 5.00 L containing 4.15 g of Helium at 298 K
      (b) 10.0 L containing 56.2 g Argon at 303 K

    2. Write down the Born-Haber cycle for the formation of CaCl2

    1. 28 g of Nitrogen and 6 g of hydrogen were mixed in a 1 litre closed container. At equilibrium 17 g NH3 was produced. Calculate the weight of nitrogen, hydrogen at equilibrium.

    2. How would you estimate the percentage of phospherous us in an organic compound?

    1. Answer the following.
      (i) Predict the major product formed when HCI is added to iso-butylene,
      (ii) What happens when CH3-Br is treated with KCN?
      (iii) Identify the chiral molecule in the following pair.

      (iv) Arrange the compounds in the order of I reactivity towards SN2 displacement. 2-Bromo-2-methylbutane, I-Bromopentane, 2-Bromo pentane.

    2. Mention the standards prescribed by BIS for quality of drinking water.

*****************************************

Reviews & Comments about 11th Standard Chemistry Revision Test Model Question Paper 2019

Write your Comment