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Complete combustion of 4.70 g of a hydrocarbon produced 15.0 g of CO₂ and 5.38 g of H₂O. What is the empirical formula for the hydrocarbon? Insert subscripts as necessary. 5 empirical formula: CH

Complete combustion of 4.70 g of a hydrocarbon produced 15.0 g of CO₂ and 5.38 g of H₂O. What is the empirical formula for the hydrocarbon? Insert subscripts as necessary. 5 empirical formula: CH

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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**Determining Empirical Formula from Combustion Data** **Problem:** A complete combustion of 4.70 g of a hydrocarbon produced 15.0 g of CO₂ and 5.38 g of H₂O. What is the empirical formula for the hydrocarbon? Insert subscripts as necessary. **Solution:** Given data: - Mass of CO₂ produced = 15.0 g - Mass of H₂O produced = 5.38 g To find the empirical formula of the hydrocarbon, follow these steps: 1. **Calculate Moles of Carbon:** - Molecular weight of CO₂ = 44.01 g/mol - Moles of CO₂ = \( \frac{15.0 \text{ g}}{44.01 \text{ g/mol}} \) - Each mole of CO₂ contains 1 mole of carbon. - Moles of carbon = Moles of CO₂ 2. **Calculate Moles of Hydrogen:** - Molecular weight of H₂O = 18.02 g/mol - Moles of H₂O = \( \frac{5.38 \text{ g}}{18.02 \text{ g/mol}} \) - Each mole of H₂O contains 2 moles of hydrogen. - Moles of hydrogen = 2 × Moles of H₂O 3. **Determine Empirical Formula:** - Divide the moles of each element by the smallest number of moles calculated. - Use the resulting ratio to determine the empirical formula. **Empirical Formula:** CH (To be determined based on calculations). **Note:** Ensure that calculations are carried out to determine the correct subscripts for the empirical formula.
Transcribed Image Text:**Determining Empirical Formula from Combustion Data** **Problem:** A complete combustion of 4.70 g of a hydrocarbon produced 15.0 g of CO₂ and 5.38 g of H₂O. What is the empirical formula for the hydrocarbon? Insert subscripts as necessary. **Solution:** Given data: - Mass of CO₂ produced = 15.0 g - Mass of H₂O produced = 5.38 g To find the empirical formula of the hydrocarbon, follow these steps: 1. **Calculate Moles of Carbon:** - Molecular weight of CO₂ = 44.01 g/mol - Moles of CO₂ = \( \frac{15.0 \text{ g}}{44.01 \text{ g/mol}} \) - Each mole of CO₂ contains 1 mole of carbon. - Moles of carbon = Moles of CO₂ 2. **Calculate Moles of Hydrogen:** - Molecular weight of H₂O = 18.02 g/mol - Moles of H₂O = \( \frac{5.38 \text{ g}}{18.02 \text{ g/mol}} \) - Each mole of H₂O contains 2 moles of hydrogen. - Moles of hydrogen = 2 × Moles of H₂O 3. **Determine Empirical Formula:** - Divide the moles of each element by the smallest number of moles calculated. - Use the resulting ratio to determine the empirical formula. **Empirical Formula:** CH (To be determined based on calculations). **Note:** Ensure that calculations are carried out to determine the correct subscripts for the empirical formula.
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