Empirical and molecular formula calculations and quantitative analysis basics - One Line Questions

1. If the molecular formula of a compound is (CH2O)n, and its molecular weight is 180 g/mol, what is the value of n? (Atomic masses: C=12, H=1, O=16) — 6
2. If the empirical formula is CH2 and the molecular formula is C3H6, what is the factor 'n' in the molecular formula (Empirical Formula)n? — 3
3. The empirical formula of glucose is CH2O. What is the ratio of carbon atoms to hydrogen atoms in a glucose molecule? — 1:2
4. If the molecular formula of a compound is twice its empirical formula, what is the ratio of their molecular weights? — 2:1
5. If a compound has a molecular formula that is three times its empirical formula, the ratio of their molecular weights is: — 3:1
6. If a compound's molecular formula is three times its empirical formula, the ratio of their molecular weights is: — 3:1
7. In the determination of the empirical formula, if the mole ratios are 0.5 : 1 : 0.25, what is the simplest whole-number ratio? — 2:4:1
8. What is the percentage composition of hydrogen in water (H2O)? (Atomic masses: H=1, O=16) — 22.22%
9. What is the percentage of potassium in potassium permanganate (KMnO4)? (Atomic masses: K=39, Mn=55, O=16) — 24.7%
10. What is the percentage of nitrogen in ammonia (NH3)? (Atomic masses: N=14, H=1) — 82.35%
11. What is the percentage of hydrogen in ethane (C2H6)? (Atomic masses: C=12, H=1) — 16.67%
12. What is the percentage of nitrogen in ammonium nitrate (NH4NO3)? (Atomic masses: N=14, H=1, O=16) — 35.0%
13. What is the percentage by mass of chlorine in carbon tetrachloride (CCl4)? (Atomic masses: C=12, Cl=35.5) — 75.76%
14. What is the percentage composition of carbon in methane (CH4)? (Atomic masses: C=12, H=1) — 92.3%
15. What is the percentage of oxygen by mass in carbon dioxide (CO2)? (Atomic masses: C=12, O=16) — 72.73%
16. What is the percentage composition of oxygen in ozone (O3)? (Atomic mass: O=16) — 100%
17. What is the percentage composition of phosphorus in phosphoric acid (H3PO4)? (Atomic masses: H=1, P=31, O=16) — 18.9%
18. What is the percentage of sulfur in sulfuric acid (H2SO4)? (Atomic masses: H=1, S=32, O=16) — 32.7%
19. A sample of an organic compound has a molar mass of 78 g/mol. If its empirical formula is C2H2, what is its molecular formula? — C6H6
20. What is the empirical formula of a compound containing 60% carbon, 8% hydrogen, and 32% oxygen by mass? (Atomic masses: C=12, H=1, O=16) — C3H4O2
21. A compound has the empirical formula C2H5. If its molecular weight is 58 g/mol, what is its molecular formula? — C4H10
22. A compound has the empirical formula C2H6O and a molecular weight of 46 g/mol. What is its molecular formula? — C2H6O
23. The empirical formula of a compound is C3H4O2. If its molecular weight is 72 g/mol, what is its molecular formula? — C3H4O2
24. The molecular formula of a compound is C3H6. What is its empirical formula? — CH2
25. A compound with the empirical formula C3H8 has a molecular weight of 44 g/mol. What is its molecular formula? — C3H8
26. If the molecular formula of a compound is C4H10, what is its empirical formula? — C2H5
27. A compound has an empirical formula C4H4O. If its molecular weight is 136 g/mol, what is its molecular formula? — C12H12O3
28. A compound has the empirical formula C4H8O2 and a molecular weight of 144 g/mol. What is its molecular formula? — C8H16O4
29. A compound has an empirical formula C5H10O and a molecular weight of 86 g/mol. What is its molecular formula? — C5H10O
30. A compound has an empirical formula C5H12. If its molecular weight is 72 g/mol, what is its molecular formula? — C5H12
31. What is the empirical formula of a compound that has the molecular formula C6H12O6? — CH2O
32. What is the empirical formula of a compound with the molecular formula C6H6? — CH
33. A substance has an empirical formula CCl2 and a molecular weight of 147 g/mol. What is its molecular formula? (Atomic masses: C=12, Cl=35.5) — C3Cl6
34. A compound has an empirical formula CH. If its molecular weight is 26 g/mol, what is its molecular formula? — C2H2
35. A compound contains 88.8% carbon and 11.2% hydrogen by mass. What is its empirical formula? (Atomic masses: C=12, H=1) — CH2
36. A compound contains 75% carbon and 25% hydrogen by mass. What is its empirical formula? (Atomic masses: C=12, H=1) — CH3
37. The combustion of 0.1 mol of an organic compound yields 0.3 mol of CO2 and 0.4 mol of H2O. What is the empirical formula of the compound? — C3H4
38. A compound has an empirical formula CH2O and a molecular weight of 60 g/mol. What is its molecular formula? — C2H4O2
39. If a compound contains 40% carbon, 6.67% hydrogen, and 53.33% oxygen by mass, what is its empirical formula? — CH2O
40. A compound contains 2.4 g of carbon, 0.4 g of hydrogen, and 3.2 g of oxygen. What is its empirical formula? — CH2O
41. A sample of a compound contains 0.5 mol of carbon, 1.0 mol of hydrogen, and 0.25 mol of oxygen. What is its empirical formula? — C2H4O
42. A compound contains 40.0% carbon, 6.7% hydrogen, and 53.3% oxygen by mass. Its molecular weight is 180 g/mol. What is its molecular formula? — C6H12O6
43. A compound contains 80% carbon and 20% hydrogen by mass. If its empirical formula is CH3, what is its molecular formula? — C2H6
44. Which of the following is NOT a step in determining the empirical formula from percentage composition? — Divide by the largest molar mass.
45. Which of the following represents the simplest whole-number ratio of atoms of each element present in a compound? — Empirical Formula
46. A compound contains 30.43% nitrogen and 69.57% oxygen by mass. What is its empirical formula? (Atomic masses: N=14, O=16) — NO2
47. A compound contains 50% sulfur and 50% oxygen by mass. What is its empirical formula? (Atomic masses: S=32, O=16) — SO2
48. A compound contains 3.2 g of sulfur and 4.8 g of oxygen. What is its empirical formula? (Atomic masses: S=32, O=16) — SO2
49. In quantitative analysis, what is the primary goal of determining the empirical formula? — To find the simplest whole-number ratio of elements.
50. In the combustion analysis of an organic compound, what is typically collected and measured to determine the amount of carbon? — Carbon Dioxide (CO2)
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