Which of the following 100.0-g samples contains the greatest number of oxygen atoms? a. H2O b. N2O C. СзН6O2 d. CO2 e. All of the samples have the same number of oxygen atoms

To determine which sample contains the greatest number of oxygen atoms, we must calculate how many moles of each compound are present in a 100.0-g sample, and then calculate the number of oxygen atoms based on the formula of each compound.

### Steps:
1. **Calculate the molar mass** of each compound.
2. **Determine the number of moles** of each compound in a 100.0-g sample.
3. **Calculate the number of oxygen atoms** in each sample by multiplying the number of moles by the number of oxygen atoms per molecule.

### a. **H₂O** (Water)
- Molar mass of H₂O: \( 2(1.01) + 16.00 = 18.02 \, \text{g/mol} \)
- Moles of H₂O in 100.0 g: \( \frac{100.0}{18.02} = 5.55 \, \text{mol} \)
- Oxygen atoms: \( 5.55 \, \text{mol} \times 1 \, \text{O} \, \text{atom per molecule} = 5.55 \, \text{mol O atoms} \)

### b. **N₂O** (Nitrous oxide)
- Molar mass of N₂O: \( 2(14.01) + 16.00 = 44.02 \, \text{g/mol} \)
- Moles of N₂O in 100.0 g: \( \frac{100.0}{44.02} = 2.27 \, \text{mol} \)
- Oxygen atoms: \( 2.27 \, \text{mol} \times 1 \, \text{O} \, \text{atom per molecule} = 2.27 \, \text{mol O atoms} \)

### c. **C₃H₆O₂** (Propane-1,2-diol)
- Molar mass of C₃H₆O₂: \( 3(12.01) + 6(1.01) + 2(16.00) = 74.08 \, \text{g/mol} \)
- Moles of C₃H₆O₂ in 100.0 g: \( \frac{100.0}{74.08} = 1.35 \, \text{mol} \)
- Oxygen atoms: \( 1.35 \, \text{mol} \times 2 \, \text{O} \, \text{atoms per molecule} = 2.70 \, \text{mol O atoms} \)

### d. **CO₂** (Carbon dioxide)
- Molar mass of CO₂: \( 12.01 + 2(16.00) = 44.01 \, \text{g/mol} \)
- Moles of CO₂ in 100.0 g: \( \frac{100.0}{44.01} = 2.27 \, \text{mol} \)
- Oxygen atoms: \( 2.27 \, \text{mol} \times 2 \, \text{O} \, \text{atoms per molecule} = 4.54 \, \text{mol O atoms} \)

### e. **Comparison**
- H₂O: 5.55 mol O atoms
- N₂O: 2.27 mol O atoms
- C₃H₆O₂: 2.70 mol O atoms
- CO₂: 4.54 mol O atoms

### Conclusion:
The sample that contains the greatest number of oxygen atoms is **H₂O** with **5.55 moles of oxygen atoms**.

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Here are 5 related questions for further exploration:
1. How do you calculate the number of atoms in a given mole of a substance?
2. What is Avogadro's number and how is it used in these calculations?
3. How would the calculation change if the sample size was different?
4. How do molecular structure and bonding affect the physical properties of these compounds?
5. Why does water contain the most oxygen atoms despite its low molar mass?

**Tip:** When calculating atoms in a compound, always consider the molecular formula and the number of each type of atom within that formula.

Which of the following 100.0-g samples contains the greatest number of oxygen atoms? a. H2O b. N2O C. С3Н6O2 d. CO2 e. All of the samples have the same number of oxygen atoms

Learn how to determine which 100.0-g sample contains the greatest number of oxygen atoms. Explore stoichiometry and molar mass calculations for H2O, N2O, C3H6O2, and CO2, using step-by-step methods. Suitable for high school students in Grades 10-12.

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