Mole Concept and Stoichiometry Quiz - ICSE Class 10 Chemistry

Free practice quiz: Mole Concept and Stoichiometry (ICSE Class 10 Chemistry). 47 multiple-choice questions with answers and explanations. Play online, no sign-up needed.

This ICSE Class 10 Chemistry practice quiz has 47 multiple-choice questions on Mole Concept and Stoichiometry, and 47 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. A compound has an empirical formula CH2O. If its molar mass is 180 g/mol, what is its molecular formula?

   1. C3H6O3
   2. C6H12O6
   3. CH2O
   4. C2H4O2
   Show answer

   Answer: B. C6H12O6

   The empirical formula mass of CH2O is 12 + 2(1) + 16 = 30 g/mol. The ratio of the molar mass to the empirical formula mass is 180 / 30 = 6. Therefore, the molecular formula is (CH2O)6, which is C6H12O6.

2. When 2 moles of hydrogen gas react with 1 mole of oxygen gas, how many moles of water are produced according to the equation 2H2 + O2 -> 2H2O?

   1. 1 mole
   2. 2 moles
   3. 3 moles
   4. 4 moles
   Show answer

   Answer: B. 2 moles

   The balanced equation shows a 2:1 mole ratio between hydrogen and oxygen, producing 2 moles of water. Since we have 2 moles of H2 and 1 mole of O2, both reactants are consumed completely according to the stoichiometry. Therefore, 2 moles of water are produced.

3. What is the number of oxygen molecules in 11.2 L of oxygen gas at STP?

   1. 6.022 x 10^23
   2. 1.2044 x 10^24
   3. 3.011 x 10^23
   4. 1.5055 x 10^23
   Show answer

   Answer: C. 3.011 x 10^23

   At STP, 1 mole of any gas occupies 22.4 L. 11.2 L of oxygen gas is equal to 11.2 L / 22.4 L/mol = 0.5 moles of oxygen gas (O2). Number of molecules = moles * Avogadro's number = 0.5 mol * 6.022 x 10^23 molecules/mol = 3.011 x 10^23 molecules.

4. What is the number of moles in 64 g of O2? (Molar mass of O2 = 32 g/mol)

   1. 1 mole
   2. 2 moles
   3. 3 moles
   4. 4 moles
   Show answer

   Answer: B. 2 moles

   Moles of O2 = Mass of O2 / Molar mass of O2 = 64 g / 32 g/mol = 2 moles.

5. If 10 g of a substance has 0.1 moles, what is its molar mass?

   1. 10 g/mol
   2. 100 g/mol
   3. 0.1 g/mol
   4. 1 g/mol
   Show answer

   Answer: B. 100 g/mol

   Molar mass = Mass / Moles = 10 g / 0.1 mol = 100 g/mol.

More questions in this quiz

Answers and explanations are in the full quiz.

1. What is the number of moles of oxygen atoms in 5 moles of calcium phosphate (Ca3(PO4)2)?
2. If 10 grams of CaCO3 are heated, what mass of CaO is produced? (Molar mass of CaCO3 = 100 g/mol, Molar mass of CaO = 56 g/mol)
3. What is the volume occupied by 4.4 g of CO2 at STP? (Molar mass of CO2 = 44 g/mol)
4. In the reaction N2 + 3H2 <=> 2NH3, if 1 mole of N2 reacts with excess H2, how many moles of NH3 are produced?
5. A 10 L container holds 0.5 moles of a gas at STP. What is the molar mass of the gas if the total mass of the gas is 11 g?
6. What is the percentage by mass of sulfur in sulfuric acid (H2SO4)? (Atomic masses: H=1, S=32, O=16)
7. How many grams of sodium chloride (NaCl) are needed to prepare 500 mL of a 0.2 M solution? (Molar mass of NaCl = 58.44 g/mol)
8. What is the number of moles of hydrogen atoms in 18 g of water (H2O)? (Molar mass of H2O = 18 g/mol)
9. A sample of a compound contains 40% carbon, 6.67% hydrogen, and 53.33% oxygen by mass. If the molar mass of the compound is 180 g/mol, what is its molecular formula?
10. What is the mass of 3.01 x 10^23 atoms of carbon? (Atomic mass of carbon = 12 g/mol)
11. Consider the reaction: Zn + 2HCl -> ZnCl2 + H2. If 6.5 g of zinc reacts with excess hydrochloric acid, what volume of hydrogen gas is produced at STP? (Molar mass of Zn = 65 g/mol, Molar volume at STP = 22.4 L/mol)
12. What is the number of moles of oxygen atoms in 0.5 moles of ozone (O3)?
13. If 4 moles of H2 react with 2 moles of O2 to form water (2H2 + O2 -> 2H2O), which is the limiting reactant and how many moles of water are produced?
14. What is the number of moles of solute in 250 mL of a 0.4 M solution?
15. Calculate the mass of 1.5 moles of methane (CH4). (Molar mass of CH4 = 16 g/mol)
16. In the reaction C + O2 -> CO2, if 12 g of carbon reacts with 32 g of oxygen, what is the mass of CO2 produced? (Molar mass of C = 12 g/mol, O2 = 32 g/mol, CO2 = 44 g/mol)
17. The empirical formula of glucose is CH2O. What is its molecular formula if its molar mass is 180 g/mol?
18. How many grams of oxygen are required to react completely with 5 moles of hydrogen to form water (2H2 + O2 -> 2H2O)? (Molar mass of O2 = 32 g/mol)
19. What is the number of moles of water molecules in 90 g of water? (Molar mass of H2O = 18 g/mol)
20. A compound has the empirical formula C2H5. If its molar mass is 58 g/mol, what is its molecular formula?
21. What is the molar concentration (molarity) of a solution containing 29.25 g of NaCl in 250 mL of solution? (Molar mass of NaCl = 58.5 g/mol)
22. In the reaction Mg + 2HCl -> MgCl2 + H2, if 24.3 g of Mg reacts with excess HCl, what volume of H2 gas is produced at STP? (Molar mass of Mg = 24.3 g/mol, Molar volume at STP = 22.4 L/mol)
23. What is the number of moles of hydrogen atoms in 2 moles of NH3?
24. If 2 moles of A react with 3 moles of B to form 1 mole of C, and the reaction is A + 2B -> C, what is the limiting reactant and how much C is formed?
25. Calculate the number of grams of oxygen in 180 g of glucose (C6H12O6). (Molar mass of C6H12O6 = 180 g/mol)
26. In the reaction 2Na + Cl2 -> 2NaCl, if 46 g of sodium reacts with 71 g of chlorine, what is the mass of sodium chloride produced? (Molar mass of Na = 23 g/mol, Cl2 = 71 g/mol, NaCl = 58.5 g/mol)
27. What is the number of molecules in 0.5 moles of sulfuric acid (H2SO4)?
28. A sample of a compound has 80% carbon and 20% hydrogen by mass. If its empirical formula mass is 15 g/mol, what is its empirical formula?
29. What is the mass of 3 moles of sodium (Na)? (Atomic mass of Na = 23 g/mol)
30. What is the empirical formula of a compound that contains 75% carbon and 25% hydrogen by mass?
31. Consider the reaction: 2Al + 3CuSO4 -> Al2(SO4)3 + 3Cu. If 5.4 g of aluminum reacts with excess copper(II) sulfate, what mass of copper is produced? (Molar mass of Al = 27 g/mol, Cu = 63.5 g/mol)
32. What is the molar mass of a gas if 2.8 g of the gas occupies 5.6 L at STP?
33. What is the number of water molecules in 18 g of water?
34. What is the percentage of oxygen by mass in potassium nitrate (KNO3)? (Atomic masses: K=39, N=14, O=16)
35. In the reaction N2 + 3H2 <=> 2NH3, if 1 mole of N2 reacts with 3 moles of H2, how many moles of NH3 are produced?
36. What is the number of moles of nitrogen atoms in 2 moles of ammonia (NH3)?
37. How many grams of water can be produced from the reaction of 2 moles of hydrogen gas with 1 mole of oxygen gas? (Molar mass of H2O = 18 g/mol)
38. What is the empirical formula of a compound that is 85.7% carbon and 14.3% hydrogen by mass?
39. What is the number of moles of oxygen atoms in 0.1 moles of carbon dioxide (CO2)?
40. If 12 g of carbon reacts with 16 g of oxygen, what mass of carbon monoxide (CO) is produced? (Molar mass of C = 12 g/mol, O = 16 g/mol, CO = 28 g/mol)
41. What is the volume occupied by 44 g of N2 gas at STP? (Molar mass of N2 = 28 g/mol)
42. What is the mass of 2 moles of sulfuric acid (H2SO4)? (Molar mass of H2SO4 = 98 g/mol)

More quizzes

• Organic Chemistry▶ Play
• Periodic Properties & Variations▶ Play
• Periodic Table, Periodic Properties and Variations of Properties▶ Play
• Study of Compounds – Ammonia▶ Play
• Study of Compounds – Nitric Acid▶ Play
• Study of Compounds – Sulphuric Acid▶ Play

Browse all Chemistry quizzes

More to play