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The burning of propane gas is given by the equation: C,H,(g) + 50,(g) → 3CO,(g) + 4H,O(g) Consider burning 1 moles of propane in 10 moles of oxygen from the atmosphere. What is the limiting reactant in this reaction, and how many moles of carbon dioxide and water are formed? 8. Oxygen is the limiting reagent; you'll make 3 moles of CO, and 4 moles of H,0. Oxygen is the limiting reagent; you'll make 6 moles of CO, and 8 moles of H,0. Propane is the limiting reagent; you'll make 3 moles of CO, and 4 moles of H,O. Propane is the limiting reagent; you'll make 9 moles of CO, and 12 moles of H,0.

The burning of propane gas is given by the equation: C,H,(g) + 50,(g) → 3CO,(g) + 4H,O(g) Consider burning 1 moles of propane in 10 moles of oxygen from the atmosphere. What is the limiting reactant in this reaction, and how many moles of carbon dioxide and water are formed? 8. Oxygen is the limiting reagent; you'll make 3 moles of CO, and 4 moles of H,0. Oxygen is the limiting reagent; you'll make 6 moles of CO, and 8 moles of H,0. Propane is the limiting reagent; you'll make 3 moles of CO, and 4 moles of H,O. Propane is the limiting reagent; you'll make 9 moles of CO, and 12 moles of H,0.

Introductory Chemistry: A Foundation
Introductory Chemistry: A Foundation
9th Edition
ISBN:9781337399425
Author:Steven S. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Donald J. DeCoste
Chapter9: Chemical Quantities
Section: Chapter Questions
Problem 43QAP: Consider the equation: 2A+B5C. If 10.0 g of A reacts with 5.00 g of B. how is the limiting reactant...
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9. Which option best explains the difference between the theoretical and actual yield in a chemical reaction? The actual yield from a chemical reaction is almost always a percentage of the reaction's theoretical yield. The amount of products formed is determined by which reactant will be used up first, based on the balanced equation for the reaction. The theoretical yield of products can be determined from the quantity of the limiting reactant. The limiting reagent controls a reaction's theoretical yield, but side reactions and human error may cause the actual yield to vary.
Transcribed Image Text:9. Which option best explains the difference between the theoretical and actual yield in a chemical reaction? The actual yield from a chemical reaction is almost always a percentage of the reaction's theoretical yield. The amount of products formed is determined by which reactant will be used up first, based on the balanced equation for the reaction. The theoretical yield of products can be determined from the quantity of the limiting reactant. The limiting reagent controls a reaction's theoretical yield, but side reactions and human error may cause the actual yield to vary.
The burning of propane gas is given by the equation: C;H,(g) + 50,(g) – 3CO,(g) + 4H,0(g) Consider burning 1 moles of propane in 10 moles of oxygen from the atmosphere. What is the limiting reactant in this reaction, and how many moles of carbon dioxide and water are formed? 8 Oxygen is the limiting reagent; you'll make 3 moles of CO, and 4 moles of H,0. Oxygen is the limiting reagent; you'll make 6 moles of CO, and 8 moles of H,O. Propane is the limiting reagent; you'll make 3 moles of CO, and 4 moles of H,0. Propane is the limiting reagent; you'll make 9 moles of CO, and 12 moles of H,0.
Transcribed Image Text:The burning of propane gas is given by the equation: C;H,(g) + 50,(g) – 3CO,(g) + 4H,0(g) Consider burning 1 moles of propane in 10 moles of oxygen from the atmosphere. What is the limiting reactant in this reaction, and how many moles of carbon dioxide and water are formed? 8 Oxygen is the limiting reagent; you'll make 3 moles of CO, and 4 moles of H,0. Oxygen is the limiting reagent; you'll make 6 moles of CO, and 8 moles of H,O. Propane is the limiting reagent; you'll make 3 moles of CO, and 4 moles of H,0. Propane is the limiting reagent; you'll make 9 moles of CO, and 12 moles of H,0.
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