Mole Concept, Class 11 Chemistry NCERT Solutions

1. There will be total 20  MCQ in this test.
2. Please keep a pen and paper ready for rough work but keep your books away.
3. The test will consist of only objective type multiple choice questions requiring students to mouse-click their correct choice of the options against the related question number.
4. No negative marking for incorrect choice.
5. Please click on “Finish the Test” when you want to exit.
6. All the best – Happy Studying.

1. Vapour density of a gas is 22. Its molecular mass will be:

33g

44g

22g

11g

Your comments:

Question 1 of 21

2. What is the mass of 0.20 mole of C₂H₅OH (ethanol)?

46 g

23 g

4.6 g

none of these

Your comments:

Question 2 of 21

3. Consider the reaction between hydrogen and oxygen gases to form water. Which of the following is/are not conserved in the reaction?
2H₂(g) + O₂(g) → 2H₂O(l)

Atoms

Mass

Both moles of molecules and moles of atoms

Moles of molecules

Your comments:

Question 3 of 21

4. How many moles of NaCl should be dissolved in 100 mL of water to get 0.2 M solution?

0.2

0.02

0.01

0.1

Your comments:

Question 4 of 21

5. Molarity of NaOH in a solution prepared by dissolving 4 g of NaOH in enough water to form 250 ml of solution is:

1.4 M

0.45 M

0.4 M

4.1 M

Your comments:

Question 5 of 21

6. Number of atoms present in 52 g of helium is:
(N_A is Avogadro’s constant Gram atomic mass of He is 4 g)

26 X N_A

N_A

13 X N_A

52 Χ N_A

Your comments:

Question 6 of 21

7. 18 g of glucose (C₆H₁₂O₆) is present in 1000 g of an aqueous solution of glucose. The molality of this solution is:

1m

0.1m

1.1m

0.5m

Your comments:

Question 7 of 21

8. Atomic mass of Cl is 35.5 g. Calculate the mass of 4.50 moles of chlorine gas, Cl₂.

6.34 g

4.5 g

160 g

319.5 g

Your comments:

Question 8 of 21

9. Atomic mass of bromine is 80 g. The mass of four moles of molecular bromine (Br₂) is:

80 g

40 g

640 g

320 g

Your comments:

Question 9 of 21

10. Number of nitrogen atoms present in 1.4 g of N₂:

6.023 X 10₂₂

6.023 X 10₂₃

3.012 X 10₂₃

3.012 X 10₂₂

Your comments:

Question 10 of 21

11. Volume of 17g of NH₃ at N.T.P. will be

22.4 L

2.24 L

4.48 L

44.8 L

Your comments:

Question 11 of 21

12. Mass of one atom of calcium is:

A

B

C

D

Your comments:

Question 12 of 21

13. Which of the following has maximum number of moles?

1g of O₂

1g of H₂

1g of Cl₂

1g of N₂

Your comments:

Question 13 of 21

14. Molar mass of F₂ is 38 g. How many atoms are present in 0.147 mole of F₂?

6.02 Χ 10₂₃ atoms

8.78 Χ 10₂₂2 atoms

0.292 atoms

1.76 Χ 10₂₃ atoms

Your comments:

Question 14 of 21

15. Molar mass of F₂ is 38 g. How many atoms are present in 0.147 mole of F₂?

6.02 Χ 10₂₃ atoms

8.78 Χ 10₂₂2 atoms

0.292 atoms

1.76 Χ 10₂₃ atoms

Your comments:

Question 15 of 21

16. Number of moles of hydroxide ions in 0.3L of 0.005M solution of Ba (OH)₂ is:

0.0015

0.003

0.0050

0.0075

Your comments:

Question 16 of 21

17. Mass of 6.022 x 10²² molecules of CO₂ is about:

1.4 g

2.2 g

12 g

4.4 g

Your comments:

Question 17 of 21

18. A solution is prepared by adding 2 g of a substance A to 18 g of water. Mass percent of solute A will be:

15%

10%

20%

25%

Your comments:

Question 18 of 21

19. Which sample contains the greatest number of nitrogen atoms? (All measurements are taken at STP.)

0.40 mol N₂ (g)

40 g NH₃(g)

0.20 mol N₂O₄ (g)

80 g N₂O₄(g)

Your comments:

Question 19 of 21

20. Normality is defined as:

Number of moles of solute per litre of solution

Number of gram equivalents of solute per litre of solution

Amount of solute present in 100g of solution

Number of moles of solute per 1000g of solvent

Your comments:

Question 20 of 21

21. Atomic mass of Si is 28 g. How many silicon atoms are there in 1.00 g of silicon?

2.14 Χ 10₂₂ atoms

1.75 Χ 10₂₅ atoms

1 atom

0.0356 atoms

Your comments:

Question 21 of 21

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