CBSE Class 11 Chemistry Mole Concept MCQs

CBSE Class 11 Chemistry Mole Concept MCQs. CBSE and NCERT students can refer to the attached file. All educational material on the website has been prepared by the best teachers having more than 20 years of teaching experience in various schools. The study material available on our website for all CBSE classes and subjects have been prepared by teachers from all over the country. All study material has been carefully designed keeping into mind the latest CBSE examination trends.  

 

I. MCQ - Choose Appropriate Alternative

1. The formula, which gives the simple ratio of each kind of atoms present in the molecule of compound, is called __________. (Molecular Formula, Empirical Formula, Structural Formula)

2. The formula, which expresses the actual number of each kind of atom present in the molecule of a compound, is called __________. (Empirical Formula, Molecular Formula, Structural Formula)

3. Mole is a quantity, which has __________ particles of the substance. (One billion, 6.02 x 1023, 1.013 x 105)

4. The simplest formula of a compound that contain 81.8% carbon and 18.2% hydrogen is __________. (CH3, CH, C2H6)

5. The empirical Formula of a compound __________. (is always the same as the molecular formula, Indicates the exact composition, Indicates the simplest ratio of the atoms)

6. Very small and very large quantities are expressed in terms of __________. (significant figures, Exponential Notation, Logarithm)

7. Two moles of water contains __________ molecules. (6.02 x 1023, 1.204 x 1024, 3.01 x 1023)

8. One mole of Cl- ions contains __________ ions. (6.02 x 1023, 1.204 x 1024, 3.01 x 1023)

9. 220 gms of CO2 contains __________ moles of CO2. (One, Five, Ten)

10. In rounding off __________ figure is dropped. (First, Last, No)

11. Precision is linked with __________. (Individual measurements, Actual results, Accepted Value) 

12. Accuracy refers to how closely a measured value agrees with __________. (Individual result, Actual result, Average value)

13. 6600 contains __________ significant figures(2, 3, 4)

14. 3.7 x 104 contains __________ significant figures. (2, 3, 5)

15. 9.40 x 10-19 contains __________ significant figures. (2, 3, 5)

16. The figure 39.45 will be rounded off to __________. (39.4, 39.5, 39)

17. __________ means that the result obtained in different experiments are very close to the accepted values. (Accuracy, Precision, Significant Figure)

18. The average weight of atoms of an element as compared to the weight of one atom of carbon taken as __________ is called the atomic weight. (12, 13, 14)

19. 58.5 is __________ of NaCl. (Atomic weight, Formula Weight, Molecular Weight)

20. 18.0 a.m.u is the __________ weight of water. (Atomic, Formula, Molecular)

21. 28 gms of nitrogen will have __________ molecules. (6.02 x 1023, 12.04 x 1023, 3.01 x 1023)

22. 22.4 dm3 of CO2 is __________ 22.4 dm3 of SO2(Heavier than, Lighter than, Equal to)

23. 100 gms of water is equal to __________ moles. (5.56, 27.78, 6.25)

24. The reactions, which proceed in both the directions are called __________ reactions. (Reversible, Irreversible, Neutrilization)

25. The reactions, which proceed in forward direction only are called __________ reactions. (Reversible, Irreversible, Ionic)

26. Molecular weight is used for __________ substances. (Ionic, Non ionic, Neutral)

27. Formula weight is used for __________ substances. (Ionic, Non ionic, Neutral)

28. The modern system of measurement is called __________ system. (SI, Metric, F.P.S)

29. The S.I unit of mass is __________. (kilogram, gram, pound)

30. One mole of glucose contains __________ gms. (100, 180, 342)


II. Fill in the Blank

1. 1 mole of a gas at S.T.P occupies a volume of __________.

2. A gas occupying a volume of 22.4 dm3 at S.T.P contains __________ molecules.

3. A formula, which gives the relative number of atoms in the molecule of a compound, is called __________.

4. A formula which gives the actual number of all kinds of atoms present in the molecule of compound is termed as __________.

5. The chemical formula that not only gives the actual number of atoms but also shows the arrangement of different atoms present in the molecule is called __________.

6. Atomic weight or molecular weight expressed in grams is known as __________.

7. 2 moles of H2O contain __________ grams and __________ number of molecules.

8. Any thing that occupies space and has __________ is called matter.

9. Volume of one __________ mole of a gas at S.T.P is 22.4 cubic feet.

10. A ton mole of iron is equal to __________ tons.

11. The force with which the earth attracts a body is called the __________ of the body.

12. A pure substance contains __________ kind of molecules.

13. The smallest indivisible particle of matter is called __________.

14. The atomic number is equal to the number of __________ in nucleus.

15. The atomic mass is the total number of protons and __________ in an atom of the element.

16. The average weight of atoms of an element as compared to the weight of one atom of __________ is called the atomic mass.

17. 1.0007 contains __________ significant figures.

18. The figure 24.75 will be rounded off to __________.

19. __________ means that the readings and measurements obtained in different experiments are very close to each other.

20. __________ means that the results obtained in different experiments are very close to the accepted values.

21. The degree of a measured quantity __________ with increasing number of significant figures in it.

22. The atomic mass of sodium is __________.

23. The symbolic representation of a molecule of a compound is called __________.

24. Molecular formula of CHCl3 and its Empirical formula is __________.

25. Molecular formula of benzene is C6H6 and its empirical formula is __________.

26. 58.5 is the __________ of NaCl.

27. 4.5 gms of nitrogen will have __________ molecules.

28. 28 gms of nitrogen will have __________ molecules.

29. 2 moles of SO2 is equal to __________ gms.

30. 1000 gms of H2O is equal to __________ moles.

31. The reactions, which proceed in both directions, are called __________.

32. The reactions, which proceed in forward directions only, are called __________ reactions.

33. The __________ reactions are completed after some time.

34. 0.0006 has __________ significant figures

35. 7.40 x 108 has __________ significant figures.

36. 7 x 108 has __________ significant figures.

37. Usually Molecular formula is simple multiple of the __________.

38. 0.1 mole of H2O contains __________ molecules of H2O.

39. Mass of 3.01 x 1022 molecules of CO2 is __________.

40. __________ is the branch of science which deals with the properties, composition and structure of matter.

41. None zero digits are all __________.

42. The integer part of logarithm is called __________.

43. The decimal fraction of logarithm is called __________.

44. __________ is the amount of substance, which contains as many number of particles as there are in 12 gms of Carbon.

45. 6.02 x 1023 is called the __________.

46. The accuracy of measurement depends on the number of __________.

47. __________ is the branch of chemistry that deals with quantitative relationships among the substances undergoing chemical changes.

48. The sum of atomic weights of all the elements present in molecular formula is called the __________.

49. __________ is the sum of atomic weights of the elements represented by the Empirical formula of the compound.

50. Very small and very large quantities are expressed in terms of __________.

51. In rounding off __________ figure is dropped.

52. Mole is the quantity, which has __________ particle of the substance.

53. For three significant figures, 25.55 is rounded off to __________.

54. The S.I unit of a mass is __________.

55. Mass of 6.02 x 1023 molecules of NaCl is __________ gm.

56. 1 mole of NaOH is __________ gm of NaOH.

57. Formula weight is used for __________ substances.

58. The word S.I stands for __________.

59. 4.5 gms of water will have __________ molecules.

60. 0.0087 has __________ significant figure.

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