Table of contents

1. The Chemical World9m
- The Scientific Method
  9m
2. Measurement and Problem Solving2h 19m
3. Matter and Energy2h 15m
4. Atoms and Elements2h 33m
5. Molecules and Compounds1h 50m
6. Chemical Composition1h 23m
7. Chemical Reactions1h 43m
8. Quantities in Chemical Reactions1h 8m
9. Electrons in Atoms and the Periodic Table2h 32m
10. Chemical Bonding2h 10m
11 Gases2h 7m
12. Liquids, Solids, and Intermolecular Forces1h 11m
13. Solutions3h 1m
14. Acids and Bases2h 14m
15. Chemical Equilibrium1h 27m
16. Oxidation and Reduction1h 33m
17. Radioactivity and Nuclear Chemistry53m

6. Chemical Composition

Empirical Formula

Introduction to Chemistry

6. Chemical Composition

Empirical Formula

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Multiple Choice

Elemental analysis of a sample of an ionic compound showed 2.82 g of Na, 4.35 g of Cl, and 7.83 g of O. What is the empirical formula of the compound?

NaClO

NaClO₂

NaClO₃

NaClO₄

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Verified step by step guidance

Step 1: Begin by determining the number of moles of each element in the sample. Use the molar mass of each element to convert grams to moles. The molar mass of Na is approximately 22.99 g/mol, Cl is approximately 35.45 g/mol, and O is approximately 16.00 g/mol.

Step 2: Calculate the moles of sodium (Na) using the formula: \( \text{moles of Na} = \frac{2.82 \text{ g}}{22.99 \text{ g/mol}} \).

Step 3: Calculate the moles of chlorine (Cl) using the formula: \( \text{moles of Cl} = \frac{4.35 \text{ g}}{35.45 \text{ g/mol}} \).

Step 4: Calculate the moles of oxygen (O) using the formula: \( \text{moles of O} = \frac{7.83 \text{ g}}{16.00 \text{ g/mol}} \).

Step 5: Determine the simplest whole number ratio of moles of each element. Divide the moles of each element by the smallest number of moles calculated in the previous steps. This will give you the subscripts for the empirical formula.