🤓 Based on our data, we think this question is relevant for Professor Khakimova's class at BELLEVUE COLLEGE.

We’re being asked to **calculate the mole fraction of CH _{4}** in a

Recall that the ** partial pressure of a gas (P_{Gas})** in a mixture is given by:

$\overline{){{\mathbf{P}}}_{{\mathbf{gas}}}{\mathbf{}}{\mathbf{=}}{{\mathbf{\chi}}}_{{\mathbf{gas}}}{{\mathbf{P}}}_{{\mathbf{total}}}}$

where **χ**** _{Gas}** = mole fraction of the gas and

The ** mole fraction of the gas** is then given by:

$\overline{){{\mathbf{\chi}}}_{{\mathbf{gas}}}{\mathbf{}}{\mathbf{=}}{\mathbf{}}\frac{\mathbf{moles}\mathbf{}\mathbf{gas}}{\mathbf{total}\mathbf{}\mathbf{moles}}}$

A mixture of CH_{4} (g) and C_{2} H_{6} (g) has a total pressure of 0.54 atm . Just enough O_{2} (g) is added to the mixture to bring about its complete combustion to CO_{2} (g) and H_{2} O(g). The total pressure of the two product gases is 2.3 atm .

Assuming constant volume and temperature, find the mole fraction of CH_{4} in the mixture.

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What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Partial Pressure concept. You can view video lessons to learn Partial Pressure. Or if you need more Partial Pressure practice, you can also practice Partial Pressure practice problems.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Khakimova's class at BELLEVUE COLLEGE.