🤓 Based on our data, we think this question is relevant for Professor McCarren's class at UIUC.

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

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

Mole fraction:

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

Solving for **partial pressure of each gas**:

- # of particles = # of moles of each gas

${\mathbf{P}}_{\mathbf{He}}\mathbf{=}{\mathbf{\chi}}_{{\mathbf{H}}_{\mathrm{e}}}{\mathbf{P}}_{\mathbf{total}}\phantom{\rule{0ex}{0ex}}\phantom{\rule{0ex}{0ex}}{\mathbf{P}}_{\mathbf{He}}\mathbf{=}\left(\frac{5}{10}\right)(1.00\mathrm{atm})$

**P _{He} = 0.50 atm**

Determine the partial pressure of each gas as shown in the figure below. Note: The relative numbers of each type of gas are depicted in the figure.

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Based on our data, we think this problem is relevant for Professor McCarren's class at UIUC.

What textbook is this problem found in?

Our data indicates that this problem or a close variation was asked in Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition. You can also practice Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition practice problems.