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Sulfur, S8, and oxygen, O2, react to form sulfur trioxide, SO3, in the (unbalanced) chemical reaction below. In a laboratory experiment, you begin with 20.1 g S8 and 29.6 g 02. You produce 43.2 g of pure SO3. What is the % yield for this reaction? S8 + 02 → SO3 + O2 SO3

Sulfur, S8, and oxygen, O2, react to form sulfur trioxide, SO3, in the (unbalanced) chemical reaction below. In a laboratory experiment, you begin with 20.1 g S8 and 29.6 g 02. You produce 43.2 g of pure SO3. What is the % yield for this reaction? S8 + 02 → SO3 + O2 SO3

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
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Sulfur, S₈, and oxygen, O₂, react to form sulfur trioxide, SO₃, in the (unbalanced) chemical reaction below. In a laboratory experiment, you begin with 20.1 g S₈ and 29.6 g O₂. You produce 43.2 g of pure SO₃. What is the % yield for this reaction? \[ \text{S}_8 + \text{O}_2 \rightarrow \text{SO}_3 \] Use the following steps to answer this question: 1. **Balance the chemical reaction** 2. **Determine the limiting reactant** (using mass to mole conversions & actual to theoretical mole comparison, considering the stoichiometric ratios in the balanced reaction) 3. **Determine the theoretical yield** (in grams) of product (based on the moles of the limit reactant and stoichiometric ratios in the balanced reaction) 4. **Calculate % yield** using the actual mass and theoretical mass of product
Transcribed Image Text:Sulfur, S₈, and oxygen, O₂, react to form sulfur trioxide, SO₃, in the (unbalanced) chemical reaction below. In a laboratory experiment, you begin with 20.1 g S₈ and 29.6 g O₂. You produce 43.2 g of pure SO₃. What is the % yield for this reaction? \[ \text{S}_8 + \text{O}_2 \rightarrow \text{SO}_3 \] Use the following steps to answer this question: 1. **Balance the chemical reaction** 2. **Determine the limiting reactant** (using mass to mole conversions & actual to theoretical mole comparison, considering the stoichiometric ratios in the balanced reaction) 3. **Determine the theoretical yield** (in grams) of product (based on the moles of the limit reactant and stoichiometric ratios in the balanced reaction) 4. **Calculate % yield** using the actual mass and theoretical mass of product
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