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Many home barbecues are fueled with propane gas (C3H8). How much carbon dioxide in kilograms is produced upon the complete combustion of 18.9 L of propane (approximate contents of one 5-gal tank)? Assume that the density of the liquid propane in the tank is 0.621g/mL.

I have no idea how to do this and I'm really stressing out on it. I'm thinking about leaving it blank. But I know I have to try.
Help me if you can, thanks!

First, you need to write a balanced equation for the combustion of C3H8. Then, you know how many liters, and you know the density, so you can calculate how many moles of C3H8 you have. Then, you can get the moles of CO2...
I hope this gets you started. Let me know if you're still stuck!!

  • chemisty -

    C3H8 + 5O2 yields 4H2O + 3CO2

    The combustion of 18.9 L of propane produces 35.1 kilograms of carbon dioxide.

  • chemisty -

    48 kg

  • chemisty -

    HeLp, A propan cylinder for a grill has an initial mass of 1.297 kg. in order to get the molecular mass of propan you collect 51.50 L of gas by water displacement at 27C. the mass of cylinder after releasing the gas is 1.203kg. if the b pressure is 15.00 psi & the water vapor pressure at 27c is 0.0352atm. I need to use this data to determine molecular mass of the propane and figure out the % error for the mass if the formula is c2h8.

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