Some Basic Concepts of Chemistry Quiz - CBSE Class 11 Science

Free practice quiz: Some Basic Concepts of Chemistry (CBSE Class 11 Science). 44 multiple-choice questions with answers and explanations. Play online, no sign-up needed.

This CBSE Class 11 Science practice quiz has 44 multiple-choice questions on Some Basic Concepts of Chemistry, and 44 of them come with an explanation. Try the 5 sample questions below (tap an option to check yourself), then play the full quiz online. No sign-up needed.

Sample questions

1. What is the SI unit of molar mass?

   1. kg
   2. g/mol
   3. mol
   4. kg/mol
   Show answer

   Answer: D. kg/mol

   Molar mass is the mass of one mole of a substance, and the SI unit of mass is kg. Therefore, the SI unit of molar mass is kg/mol.

2. Describe the process of stoichiometric calculations.

   1. Calculations involving the mass of reactants and products in a chemical reaction.
   2. Calculations involving the volume of reactants and products in a chemical reaction.
   3. Calculations involving the rate of chemical reactions.
   4. Calculations involving the temperature of chemical reactions.
   Show answer

   Answer: A. Calculations involving the mass of reactants and products in a chemical reaction.

   Stoichiometric calculations use the balanced chemical equation to relate the amounts of reactants and products.

3. Explain the concept of molar volume of a gas.

   1. The volume occupied by one mole of a gas at STP.
   2. The volume occupied by one gram of a gas at STP.
   3. The volume occupied by one kilogram of a gas at STP.
   4. The volume occupied by any amount of gas at STP.
   Show answer

   Answer: A. The volume occupied by one mole of a gas at STP.

   At standard temperature and pressure (STP), one mole of any ideal gas occupies a volume of approximately 22.4 liters.

4. Explain the concept of an empirical formula.

   1. The simplest whole-number ratio of atoms of each element in a compound.
   2. The actual number of atoms of each element in a molecule.
   3. The formula that shows the arrangement of atoms in a molecule.
   4. The formula that shows only the metallic elements in a compound.
   Show answer

   Answer: A. The simplest whole-number ratio of atoms of each element in a compound.

   The empirical formula represents the simplest whole-number ratio of atoms of different elements present in a compound.

5. Explain the difference between a pure substance and a mixture.

   1. A pure substance has a fixed composition, while a mixture does not.
   2. A pure substance has a variable composition, while a mixture does not.
   3. Pure substances and mixtures are the same.
   4. Pure substances are always solids, mixtures are always liquids.
   Show answer

   Answer: A. A pure substance has a fixed composition, while a mixture does not.

   A pure substance has a definite and constant composition, while a mixture is a combination of two or more substances.

More questions in this quiz

Answers and explanations are in the full quiz.

1. What is the number of significant figures in 0.0025?
2. Which of the following is an example of an extensive property?
3. Define Avogadro's number.
4. Explain the difference between precision and accuracy in measurement.
5. What is the law of conservation of mass?
6. Explain the concept of limiting reagent in a chemical reaction.
7. A reaction has a theoretical yield of 100g, but only produces 80g. What is the percent yield?
8. What are the differences between a mole and a molecule?
9. Explain how to determine the molecular formula of a compound given its empirical formula and molar mass.
10. What is the relationship between pressure, volume, and temperature of an ideal gas?
11. How does Dalton's atomic theory explain the law of multiple proportions?
12. What is the difference between a homogeneous and a heterogeneous mixture?
13. Explain the concept of a mole fraction.
14. A solution is prepared by dissolving 10g of solute in 90g of water. What is the mass percentage of the solute?
15. What is the difference between an atom and an ion?
16. What is the role of a catalyst in a chemical reaction?
17. What is the significance of a balanced chemical equation?
18. How many atoms are present in 2 moles of oxygen gas (O₂)?
19. What is meant by the term 'stoichiometry'?
20. Explain the concept of percentage composition of a compound.
21. What is the significance of the law of definite proportions?
22. How does Gay-Lussac's law relate to stoichiometry?
23. What is the role of significant figures in chemical calculations?
24. What are the limitations of Dalton's atomic theory?
25. Explain the concept of a standard solution.
26. What is the molarity of a solution that contains 0.2 moles of solute in 500 ml of solution?
27. What is the difference between molarity and molality?
28. Explain the concept of normality in solutions.
29. What is the mass of 0.5 moles of carbon dioxide (CO₂)? (C=12, O=16)
30. How does Avogadro's law relate to the ideal gas law?
31. What is the volume occupied by 2 moles of an ideal gas at STP?
32. What is the concept of a limiting reactant and how does it affect the yield of a reaction?
33. Describe how to calculate the percent yield of a reaction.
34. What are some factors that can affect the percent yield of a chemical reaction?
35. Explain how to convert between moles, grams, and number of particles.
36. What is the significance of the ideal gas law in chemistry?
37. What are the assumptions made in the ideal gas law?
38. Explain how deviations from ideal gas behavior occur.
39. How can the van der Waals equation be used to correct for non-ideal gas behavior?

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