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.
General Chemistry - Standalone book (MindTap Course List)
11th Edition
ISBN:9781305580343
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Chapter3: Calculations With Chemical Formulas And Equaitons
Section: Chapter Questions
Problem 3.23QP: High cost and limited availability of a reactant often dictate which reactant is limiting in a...
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Question
Please help me fix this equation so i can submit it, I am not sure where i put the wrong inputs
![81.7
mol CO₂
STARTING AMOUNT
81.7 mol CO, *
CO₂
X
81.7 g O₂
32.00 mol O₂
X
81.7
32.00
1 mol CO₂
2 mol O₂
gO₂
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:
CH4(g) + 2 O₂(g) → CO₂(g) + 2 H₂O(1)
X
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.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F2286f692-685a-4661-8fbb-20d89553ded3%2F215764a4-72e0-4ddd-8443-2012a93b73ed%2F6435sli_processed.png&w=3840&q=75)
Transcribed Image Text:81.7
mol CO₂
STARTING AMOUNT
81.7 mol CO, *
CO₂
X
81.7 g O₂
32.00 mol O₂
X
81.7
32.00
1 mol CO₂
2 mol O₂
gO₂
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:
CH4(g) + 2 O₂(g) → CO₂(g) + 2 H₂O(1)
X
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.
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