**Problem Statement:**Styrene, the building block of polystyrene, consists of only carbon (C) and hydrogen (H). If 0.624 g of styrene is burned in oxygen and produces 2.108 g of carbon dioxide (CO₂) and 0.432 g of water (H₂O), what is the empirical formula of styrene?**Empirical Formula:**[Input Box for Answer]**Exercise Explanation:**This exercise involves determining the empirical formula of styrene based on the combustion analysis data provided. When styrene is burned, it produces carbon dioxide and water, from which we can calculate the amount of carbon and hydrogen present in styrene.**Steps to Solve:**1. **Calculate the Moles of Carbon:** - Use the mass of CO₂ to find moles of carbon. - Molar Mass of CO₂ = 44.01 g/mol. - Moles of CO₂ = mass (2.108 g) / molar mass (44.01 g/mol). - Each mole of CO₂ contains one mole of C.2. **Calculate the Moles of Hydrogen:** - Use the mass of H₂O to find moles of hydrogen. - Molar Mass of H₂O = 18.02 g/mol. - Moles of H₂O = mass (0.432 g) / molar mass (18.02 g/mol). - Each mole of H₂O contains two moles of H.3. **Determine the Empirical Formula:** - Use the mole ratio of carbon to hydrogen to determine the simplest whole number ratio.This educational exercise challenges learners to apply concepts of stoichiometry and empirical formula determination.

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Answered: Styrene, the building block of…

Chemistry

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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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Styrene, the building block of polystyrene, consists of only C and H. If 0.624 g of styrene is burned in oxygen and produces 2.108 g of CO2 and 0.432 g of H2O, what is the empirical formula of styrene? Empirical formula: