A 16.0 gram sample of propane gas(C3H8) is burned according to the equationC3H8(g) + 5O2(g) →3CO2(g) + 4H2O(g).
In an enclosed container with a volume of 2.25L at atemperature of 322K.
If the sample of propane burns completely and no oxygenremains in the container, calculate the mole fractions ofCO2 and H2O.
Calculate the total pressure in the container after thereaction.
Calculate the partial pressure of CO2 andH2O in the container after the reaction.
If 12.1 grams of propane is burned in the presence of10.2 atm of oxygen at the above temperature and volume conditions,determine the theoretical yield of H2O.
