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Sulfur, S8, and oxygen, O2, react to form sulfur trioxide, S03, 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? S8 + O2 → SO3 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

Sulfur, S8, and oxygen, O2, react to form sulfur trioxide, S03, 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? S8 + O2 → SO3 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

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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How do I do this? The theoretical yield is 87.50, how do I get this?
ctober 19 – Stoichiometry in Chemical Reactions ulfur, S3, and oxygen, O2, react to form sulfur trioxide, S e (unbalanced) chemical reaction below. In a laboratory <periment, you begin with 20.1 g Sg and 29.6 g O2. You 3.2 g of pure SO3. What is the % yield for this reaction? pur work with correct formatting. Sg + O2 SO3 tep #1 – Balance the chemical reaction S3 + 12 O2 → 8 SO3 tep #2 – Determine the limiting reactant herefore, O, is the limiting reactant and S3 is the excess tep #3 – Determine the theoretical yield (in grams) of pr tep #4- Calculate % yield Therefore, this reaction has an 87.5% yield of SC
Transcribed Image Text:ctober 19 – Stoichiometry in Chemical Reactions ulfur, S3, and oxygen, O2, react to form sulfur trioxide, S e (unbalanced) chemical reaction below. In a laboratory <periment, you begin with 20.1 g Sg and 29.6 g O2. You 3.2 g of pure SO3. What is the % yield for this reaction? pur work with correct formatting. Sg + O2 SO3 tep #1 – Balance the chemical reaction S3 + 12 O2 → 8 SO3 tep #2 – Determine the limiting reactant herefore, O, is the limiting reactant and S3 is the excess tep #3 – Determine the theoretical yield (in grams) of pr tep #4- Calculate % yield Therefore, this reaction has an 87.5% yield of SC
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 Sg and 29.6 g 02. You produce 43.2 g of pure SO3. What is the % yield for this reaction? S8 + 02 → SO3 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 Sg and 29.6 g 02. You produce 43.2 g of pure SO3. What is the % yield for this reaction? S8 + 02 → SO3 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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