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What is the empirical formula of the following compound given the following data? The sample contains 0.130g of nitrogen and 0.370g oxygen. (1) NO2 0 1 05 4 2 3 (2) N₂O3 (3) N₂O4 (4) N₂O5 (5) NO

What is the empirical formula of the following compound given the following data? The sample contains 0.130g of nitrogen and 0.370g oxygen. (1) NO2 0 1 05 4 2 3 (2) N₂O3 (3) N₂O4 (4) N₂O5 (5) NO

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**Empirical Formula Determination** **Question:** What is the empirical formula of the following compound given the following data? The sample contains 0.130g of nitrogen and 0.370g of oxygen. **Options:** 1. \( \text{NO}_2 \) 2. \( \text{N}_2\text{O}_3 \) 3. \( \text{N}_2\text{O}_4 \) 4. \( \text{N}_2\text{O}_5 \) 5. \( \text{NO} \) ### Multiple Choice Answers: - ○ 1 - ○ 5 - ○ 4 - ○ 2 - ○ 3 **Explanation/Discussion:** To determine the empirical formula, we must first convert the given masses to moles using the molar masses of nitrogen (N) and oxygen (O). 1. **Calculate moles of Nitrogen:** - Molar mass of N = 14.01 g/mol - Moles of N = \( \frac{0.130 \text{ g}}{14.01 \text{ g/mol}} \) ≈ 0.00928 mol 2. **Calculate moles of Oxygen:** - Molar mass of O = 16.00 g/mol - Moles of O = \( \frac{0.370 \text{ g}}{16.00 \text{ g/mol}} \) ≈ 0.02313 mol 3. **Determine the simplest whole number ratio:** - Ratio of N:O = \( \frac{0.00928}{0.00928} : \frac{0.02313}{0.00928} \) ≈ 1 : 2.5 - To get whole numbers, multiply by 2: 2 : 5 Hence, the empirical formula is \( \text{N}_2\text{O}_5 \). Therefore, the correct option is 4. \( \text{N}_2\text{O}_5 \).
Transcribed Image Text:**Empirical Formula Determination** **Question:** What is the empirical formula of the following compound given the following data? The sample contains 0.130g of nitrogen and 0.370g of oxygen. **Options:** 1. \( \text{NO}_2 \) 2. \( \text{N}_2\text{O}_3 \) 3. \( \text{N}_2\text{O}_4 \) 4. \( \text{N}_2\text{O}_5 \) 5. \( \text{NO} \) ### Multiple Choice Answers: - ○ 1 - ○ 5 - ○ 4 - ○ 2 - ○ 3 **Explanation/Discussion:** To determine the empirical formula, we must first convert the given masses to moles using the molar masses of nitrogen (N) and oxygen (O). 1. **Calculate moles of Nitrogen:** - Molar mass of N = 14.01 g/mol - Moles of N = \( \frac{0.130 \text{ g}}{14.01 \text{ g/mol}} \) ≈ 0.00928 mol 2. **Calculate moles of Oxygen:** - Molar mass of O = 16.00 g/mol - Moles of O = \( \frac{0.370 \text{ g}}{16.00 \text{ g/mol}} \) ≈ 0.02313 mol 3. **Determine the simplest whole number ratio:** - Ratio of N:O = \( \frac{0.00928}{0.00928} : \frac{0.02313}{0.00928} \) ≈ 1 : 2.5 - To get whole numbers, multiply by 2: 2 : 5 Hence, the empirical formula is \( \text{N}_2\text{O}_5 \). Therefore, the correct option is 4. \( \text{N}_2\text{O}_5 \).
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