Atomic and molecular masses and mole concept - One Line Questions

1. What is the concentration of ions in a 0.1 M solution of CaCl₂? — 0.3 M
2. If a solution contains 1 mole of solute and 4 moles of solvent, what is the mole fraction of the solute? — 0.2
3. What is the mole fraction of solute if 2 moles of solute are dissolved in 8 moles of solvent? — 0.2
4. If a solution has a molarity of 0.5 M and a volume of 2 liters, how many moles of solute are present? — 1 mole
5. What is the mole fraction of a solute if the mole fraction of the solvent is 0.7? — 0.3
6. What is the mole fraction of water in a solution prepared by dissolving 18 g of glucose (C₆H₁₂O₆) in 180 g of water? — 0.5
7. If 1 mole of NaCl is dissolved in water, how many moles of Na⁺ ions are produced? — 1 mole
8. How many moles are present in 18 grams of water (H₂O)? (Molar mass of H₂O ≈ 18 g/mol) — 1 mole
9. How many moles are present in 44 grams of carbon dioxide (CO₂)? (Molar mass of CO₂ ≈ 44 g/mol) — 1 mole
10. What is the number of moles in 1 kg of substance? — 1000 / Molar mass (in g/mol)
11. How many atoms are present in 1 mole of gold (Au)? — 6.022 x 10^23 atoms
12. The molar mass of a compound is numerically equal to its relative molecular mass multiplied by: — 1 g/mol
13. What is the number of moles of oxygen atoms in 2 moles of carbon dioxide (CO₂)? — 4 moles
14. What is the number of moles in 100 grams of calcium carbonate (CaCO₃)? (Atomic masses Ca=40, C=12, O=16) — 1 mole
15. What is the number of moles of hydrogen atoms in 1 mole of methane (CH₄)? — 4 moles
16. Which of the following has the smallest mass? — 1 mole of hydrogen atoms
17. Which of the following has the largest number of atoms? — 1 mole of He
18. Which of the following has the largest mass? — 1 mole of Oxygen
19. What is the atomic mass unit (amu) defined as? — 1/12th the mass of an atom of carbon-12
20. Which of the following represents the molecular mass of methane (CH₄)? — 16 amu
21. One mole of any substance contains the same number of entities (atoms, molecules, ions, etc.) as there are atoms in: — 12 grams of carbon-12
22. What is the molar mass of ammonia (NH₃)? (Atomic masses N=14, H=1) — 17 g/mol
23. How many grams of oxygen gas (O₂) are there in 2 moles of O₂? (Atomic mass O=16) — 64 g
24. What is the molar mass of ozone (O₃)? (Atomic mass O=16) — 48 g/mol
25. What is the molar mass of water (H₂O), given atomic masses H=1.008 amu, O=15.999 amu? — 18.015 g/mol
26. What is the mass of one molecule of water (H₂O)? (Atomic masses H=1, O=16, N_A = 6.022 x 10^23 mol⁻¹) — 3.0 x 10⁻²³ g
27. Which of the following has the largest number of molecules? — 18 g of H₂O
28. What is the molar mass of glucose (C₆H₁₂O₆)? (Atomic masses C=12, H=1, O=16) — 180 g/mol
29. What is the mass of 2 moles of carbon dioxide (CO₂)? (Atomic mass C=12, O=16) — 88 g
30. What is the total number of moles of atoms in 1 mole of sodium sulfate (Na₂SO₄)? — 5 moles
31. What is the mass of 0.1 moles of sodium hydroxide (NaOH)? (Atomic masses Na=23, O=16, H=1) — 4 g
32. What is the mass of 0.5 moles of sulfuric acid (H₂SO₄)? (Atomic masses H=1, S=32, O=16) — 49 g
33. What is the number of moles in 10 grams of hydrogen gas (H₂)? (Atomic mass H=1) — 5 moles
34. How many grams of NaCl are there in 0.1 moles of NaCl? (Atomic masses Na=23, Cl=35.5) — 5.85 g
35. Avogadro's number (N_A) is approximately: — 6.022 x 10^23
36. How many molecules are present in 36 grams of water (H₂O)? (Molar mass of H₂O ≈ 18 g/mol, N_A = 6.022 x 10^23 mol⁻¹) — 1.2044 x 10^24 molecules
37. What is the total number of moles of atoms in 1 mole of calcium phosphate (Ca₃(PO₄)₂)? — 13 moles
38. What is the mass of 0.2 moles of sulfuric acid (H₂SO₄)? (Atomic masses H=1, S=32, O=16) — 19.6 g
39. The term 'gram molecular mass' is synonymous with: — Molar mass
40. The mass of a substance containing N_A entities is equal to its: — Molar mass
41. The molar mass of a substance is numerically equal to its: — Molecular mass in amu
42. The term 'gram atomic mass' is synonymous with: — Molar mass of an element
43. If the empirical formula of a compound is CH₂O and its molar mass is 180 g/mol, what is its molecular formula? — C₆H₁₂O₆
44. What is the SI unit for the amount of substance? — Mole
45. Which element has an atomic mass closest to 1 amu? — Hydrogen
46. The number of moles of a substance is calculated as: — Both a and c
47. The number of moles of solute in 1 liter of solution is called: — Molarity
48. The number of moles of solute in 1 kg of solvent is called: — Molality
49. The number of moles of solute per kilogram of solvent is: — Molality
50. The relative atomic mass of an element is the ratio of the average mass of atoms of an element to: — 1/12th the mass of an atom of carbon-12
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