The partial pressure of CH4(g) is 0.175 atm, and the partial pressure of O2(g) is 0.250 atm in a mixture of the two gases. The mixture occupies a volume of 10.5 L at 65 oC. Solve all three parts of the question. 1) The mole fraction of CH4(g) is , and the mole fraction of O2(g) is . 2) The total number of moles of gas in the mixture is . 3) There are grams of CH4(g) and grams of O2(g) in the mixture.

1)

2)

3)

Explanation:

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1) In this case, given the partial pressures of both methane and oxygen we can compute the mole fraction by considering each partial pressure as shown below:

2) Now, we use the ideal gas equation to compute the total mass with the total pressure:

3) Finally, by using the mole fractions, total moles and molar masses we compute the grams of both methane and oxygen:

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> b takes place in the gas phase in an isothermal tubular reactor. the feed is one mole of a per one mole of c, an inert. the entering temperature and pressure are 427°c and 10 atm, respectively. the gas constant r = 0.08206 atm · l/mol · k.