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28 Nov 2019
A 16.0 gram sample of propane gas (C3H8) is burned according to the equation C3H8(g) + 5O2(g) â 3CO2(g) + 4H2O(g).
In an enclosed container with a volume of 2.25L at a temperature of 322K.
If the sample of propane burns completely and no oxygen remains in the container, calculate the mole fractions of CO2 and H2O.
Calculate the total pressure in the container after the reaction.
Calculate the partial pressure of CO2 and H2O in the container after the reaction.
If 12.1 grams of propane is burned in the presence of 10.2 atm of oxygen at the above temperature and volume conditions, determine the theoretical yield of H2O.
A 16.0 gram sample of propane gas (C3H8) is burned according to the equation C3H8(g) + 5O2(g) â 3CO2(g) + 4H2O(g).
In an enclosed container with a volume of 2.25L at a temperature of 322K.
If the sample of propane burns completely and no oxygen remains in the container, calculate the mole fractions of CO2 and H2O.
Calculate the total pressure in the container after the reaction.
Calculate the partial pressure of CO2 and H2O in the container after the reaction.
If 12.1 grams of propane is burned in the presence of 10.2 atm of oxygen at the above temperature and volume conditions, determine the theoretical yield of H2O.
Keith LeannonLv2
18 Nov 2019
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