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100 pts
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Question 12 of 15
4. A mixture of methane gas, \( \mathrm{CH}_{4}(\mathrm{~g}) \), and propane gas, \( \mathrm{C}_{3} \mathrm{H}_{8}(\mathrm{~g}) \), has a pressure of 0.5298 bar when placed in a sealed container.
The complete combustion of the mixture to carbon dioxide gas, \( \mathrm{CO}_{2}(\mathrm{~g}) \), and water vapor, \( \mathrm{H}_{2} \mathrm{O}(\mathrm{g}) \), was achieved by adding exactly enough oxygen gas, \( \mathrm{O}_{2}(\mathrm{~g}) \), the the container. The pressure of the product mixture in the sealed container is 2.373 bar. Calculate the mole fraction of methane in the initial mixture assuming the temperature and volume remain constant.
\[
x_{\mathrm{Cl}_{4}}=
\]
\( \square \)
