A 16.0 gram sample of propane gas (C3H8) is burned according to the equation C3H8(g) + 5O2(g)...

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Chemistry

A 16.0 gram sample of propane gas(C³H⁸) is burned according to the equationC₃H₈(g) + 5O₂(g) â†’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.

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Number of moles of propane n massmolar mass 160 g 44 gmol 036 mol C3H8g 5O2g 3CO2g 4H2Og From the balanced equation 1 mole of propane produces 3 moles of CO2 4 moles of H2O 036 mole of propane produces 3x036108 moles of CO2 4x036144 moles of H2O So total num ber of moles N 108 144 252 mole So mole fraction of CO2 is X CO2 See Answer

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