Please help me with this problem

  • Thread starter hima
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  • #1
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?

Answers and Replies

  • #2
Could you please tell us what you have done already, and where exactly you need help/don't understand?
  • #3
The questions are clear, but the problem is that we can't answer to homeworks here .
  • #4
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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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