Calculating Limiting Reagent and Percent Yield for Gasoline Combustion

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Discussion Overview

The discussion revolves around a chemistry problem involving the combustion of gasoline (octane) and the calculation of the limiting reagent, mass of carbon dioxide produced, and percent yield of the reaction. The scope includes theoretical and homework-related aspects of stoichiometry and gas laws.

Discussion Character

  • Homework-related

Main Points Raised

  • One participant requests assistance with a specific homework problem involving the combustion of gasoline, including calculations for limiting reagent and percent yield.
  • Another participant asks for clarification on what the requester has already attempted and where they specifically need help.
  • One participant notes that the questions are clear but states that homework assistance is not permitted in the forum.
  • A later reply suggests performing calculations in mole units and emphasizes the need for the density of gasoline to convert from volume to mass for further calculations.
  • Participants clarify the notation in the chemical equation, indicating that "l" stands for liquid and "g" stands for gas.

Areas of Agreement / Disagreement

Participants generally agree on the need for additional information and calculations but disagree on the appropriateness of providing direct homework help.

Contextual Notes

Limitations include the need for the density of gasoline to convert volume to mass, which is not provided. The discussion does not resolve how to approach the calculations without this information.

Who May Find This Useful

Students studying stoichiometry, combustion reactions, and those seeking to understand the concepts of limiting reagents and percent yield in chemical reactions.

hima
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please i need to solve this problem, can you help me out. thank you.
equation: 2C8H18 (l) + 25O2 (g) → 16CO2 (g) + 18H2O (l)
a)2.62kg(one gallon) of gasoline is burned with 7000.0L of oxygen gas at STP. what is the limiting reagent?
b) what mass of carbon dioxide is produced in part?
c) if 6.4 kg of carbon dioxide is collected in the lab using the amounts in part(a), what is the percent yield for this experiment?
 
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Could you please tell us what you have done already, and where exactly you need help/don't understand?
 
The questions are clear, but the problem is that we can't answer to homeworks here .
 
You would perform most of your calculations in mole units. Since your given quantity of gasoline is in gallons(a volume unit), you need to know this gasoline's density (or specific gravity, at least something to work with); the density will give you the mass, and the mass will give you the moles (obviously using suitable conversion calculations).

The "l" in your reaction means "liquid", and the "g" in your reaction means "gas"
 

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