mol CO₂ STARTING AMOUNT 81.7 81.7 mol COz * X 81.7 g 0₂ 32.00 mol O₂ X 81.7 32.00 1 mol CO₂ 2 mol O₂ g 0₂ mol O₂ = 1 mol CO₂ [Tutorial: Limiting/Excess reactant] This question will walk you through the steps of determining which reactant is limiting based on a balanced chemical equation. Step 2b: Use dimensional analysis to determine the theoretical yield of the product. Calculate the theoretical yield in moles CO₂ from the complete reaction of 81.7 grams O₂ according to the following balanced chemical equation: X CH4(g) + 2 O₂(g) → CO₂(g) + 2 H₂O(1) 1 2 mol CO₂ mol O₂ = 1 mol CO₂ Incorrect, 987 attempts remaining You seem to have specified the wrong molar mass for O₂ in your first conversion factor. Recalculate the molar mass of O₂ and then try again.
mol CO₂ STARTING AMOUNT 81.7 81.7 mol COz * X 81.7 g 0₂ 32.00 mol O₂ X 81.7 32.00 1 mol CO₂ 2 mol O₂ g 0₂ mol O₂ = 1 mol CO₂ [Tutorial: Limiting/Excess reactant] This question will walk you through the steps of determining which reactant is limiting based on a balanced chemical equation. Step 2b: Use dimensional analysis to determine the theoretical yield of the product. Calculate the theoretical yield in moles CO₂ from the complete reaction of 81.7 grams O₂ according to the following balanced chemical equation: X CH4(g) + 2 O₂(g) → CO₂(g) + 2 H₂O(1) 1 2 mol CO₂ mol O₂ = 1 mol CO₂ Incorrect, 987 attempts remaining You seem to have specified the wrong molar mass for O₂ in your first conversion factor. Recalculate the molar mass of O₂ and then try again.
Chemistry for Engineering Students
4th Edition
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Lawrence S. Brown, Tom Holme
Chapter3: Molecules, Moles, And Chemical Equations
Section: Chapter Questions
Problem 3.75PAE: 3.75 The following pictures show a molecular-scale view of a chemical reaction between the compounds...
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