Most expected three mark questions in Basic Concepts of Chemistry and Chemical Calculations - IV

11th Standard

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Chemistry

Answer any 50 questions
Time : 02:00:00 Hrs
Total Marks : 150

    Part - A

    56 x 3 = 168
  1. Balance the following reaction:
    Sb3++ Mn\({ O }_{ 4 }^{ - }\)\(\rightarrow \) Sb5++ Mn2+

  2. Define the following: (i) Element, (ii) Compound.

  3. Give two examples of elementary molecules which are (i) Monoatomic (ii) Diatomic and (iii) Polyatomic.

  4. Define a.m.u or unified atomic mass.

  5. Calculate the mass of the following atoms in a.m.u (unified atomic mass).

  6. The relative abundance of 6C12,6C13and 6C14are 98.892%, 1.108% and 2 x 10-10respectively. Calculate the average atomic mass of carbon.

  7. The relative abundance of 10Af36, 10Ar38,10.Ar40are 0.337%,0.063% and 99.6% respectively. Calculate the average atomic weight of Argon:

  8. Calculate the molecular masses of the following: KMnO4,

  9. Calculate the molecular masses of the following: NaOH

  10. Calculate the molecular masses of the following:H2C2O4.2H2O,

  11. Calculate the molecular masses of the following:C6H12O6

  12. Explain the term "mole".

  13. Calculate the number of atoms / molecules present in the following: 10 gram of mercury

  14. Calculate the number of atoms / molecules present in the following 1.8 gram of water

  15. Calculate the number of atoms / molecules present in the following 100 gram of sulphur dioxide

  16. Calculate the number of atoms / molecules present in the following 1 kg of acetic acid (CH3COOH)

  17. Calculate the number of atoms / molecules present in the following 46 gram of sodium

  18. Calculate the number of moles present in 9 grams of ethane.

  19. Calculate the volume occupied at STP by the following: 0.5 mole of methane

  20. A substance an analysis, gave the following percentage composition, Na = 43.4%, C=11.3%, 0= 43.3% calculate its empirical formula

  21. An organic compound contains the following composition by mass: C = 92.3%, H = 7.7%. At STP, 10L of the gas has the mass 11.6g. Find the molecular formula of the compound.

  22. An organic compound has the following composition by mass:C = 40.92%, H = 4.58% and the rest oxygen. The molar mass of the compound is 176g mol ". Determine the molecular formula of the compound.

  23. Mass of one atom of an element is 6.66 x 10-23 g.How many moles of element are there in 0.320 kg?

  24. What is the amount of silver oxide formed when 11.04g of silver carbonate is strongly heated? Write the balanced chemical equation for the .reaction. Ag2C03 \(\rightarrow\)2AgO + CO2.

  25. How much volume of hydrogen is liberated when 0.12g of magnesium reacts with dilute hydrochloric acid?

  26. How much volume of nitrogen and hydrogen are required-to produce 100cm3 of ammonia?

  27. Calculate the equivalent, mass of hydrated sodium carbon.

  28. Calculate the mass of sodium (in kg) present in 95 kg of a crude sample of sodium nitrate whose percentage purity is 70%.

  29. A Compound on analysis gave the following percentage composition C = 54.55%, H = 9.09%, O = 36.36%. Determine the empirical formula of the compound.

  30. Distinguish among the different physical states of matter.

  31. Define equivalent mass of a salt.

  32. How much copper can be obtained from 100 g of anhydrous copper sulphate?

  33. Calculate the equivalent mass of hydrated ferrous sulphate

  34. A sample of hydrated copper sulphate is heated to drive off the water of crystallization, cooled and reweighed 0.869 g of CuSO4.aH2O gave a residue of 0.556 g. Find the molecular formula of hydrated copper sulphate.

  35. Balance by oxidation number method:Mg +HNO3 \(\rightarrow\) Mg(NO3)2 + NO2 + H2O

  36. Explain about the classification of matter.

  37. Calculate the mass of the following atoms in amu,
    (a) Helium (mass of He = 6.641 x 10-24g)
    (b) Silver (mass of Ag = 1.790 X 10-22g)

  38. Calculate the number of atoms present in 1 Kg of gold

  39. Calculate the molar volume of 146 g of HCI gas and the number of molecules present in it

  40. Calculate the molar mass of 20 L of gas weighing 23.2 g at STP.

  41. 0.6 g of a metal gives on oxidation 1 g of its oxide. Calculate its equivalent mass

  42. How would you calculate the equivalent mass of anhydrous oxalic acid and hydrated oxalic acid.

  43. A compound on decomposition in the laboratory produces 24.5 g of nitrogen and 70 g of oxygen. Calculate the empirical formula of the compound.

  44. What is the steps involve in the calculation of molecular formula from empirical formula?

  45. What is combination reaction? Give example

  46. What is decomposition reaction? Give two examples.

  47. What is displacement reactions? Give its types. Explain with example.

  48. What is disproportionation reactions? Give example

  49. What are competitive electron transfer reaction? Give example

  50. Balance the following equation using oxidation number method.

  51. Determine the empirical formula of an oxide of iron which has 69.9% iron and 30.1% oxygen by mass

  52. In three moles of ethane (C2H6) calculate the following:
    (i) Number of moles of carbon atoms.
    (ii) Number of moles of hydrogen atoms.
    (iii) Number of molecules of ethane.

  53. Chlorine is prepared in the laboratory by treating manganese dioxide (MnO2) with aqueous hydrochloric acid according to the reaction.
    \({ 4HCl }_{ (aq) }+{ Mn }O_{ { 2 }_{ (s) } }\rightarrow 2H_{ 2 }{ O }_{ (1) }+{ MnCl }_{ { 2 }_{ (aq) } }+{ Cl }_{ { 2 }_{ (g) } }\)
    How many grams of HCI react with 5.0 g of manganese dioxide?
    (Atomic mass of Mn = 55 g).

  54. The density of water at room temperature is 1.0 g/mI. How many molecules are there in a drop of water if its volume is 0.05 ml?

  55. Balance the following equation by oxidation number method. MnO4- + Fe2+ \(\rightarrow\)  Mn2+ + Fe3+ (Acidic medium)

  56. Balance the following equation using oxidation number method
    As2S3 + HNO3 + H2\(\rightarrow\) H3AsO4 + H2SO4 + NO

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