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

$\overline{){{\mathbf{P}}}_{{\mathbf{Gas}}}{\mathbf{=}}{{\mathbf{X}}}_{\mathbf{G}\mathbf{a}\mathbf{s}}{{\mathbf{P}}}_{{\mathbf{Total}}}}\phantom{\rule{0ex}{0ex}}$

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

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

$\overline{){\mathit{m}}{\mathit{o}}{\mathit{l}}{\mathit{e}}{\mathbf{}}{\mathit{f}}{\mathit{r}}{\mathit{a}}{\mathit{c}}{\mathit{t}}{\mathit{i}}{\mathit{o}}{\mathit{n}}{\mathbf{}}{\mathbf{\left(}}{\mathit{X}}{\mathbf{\right)}}{\mathbf{=}}\frac{\mathbf{m}\mathbf{o}\mathbf{l}\mathbf{e}\mathbf{}\mathbf{o}\mathbf{f}\mathbf{}\mathbf{gas}}{\mathbf{total}\mathbf{}\mathbf{mass}}}$

The drawing below represents a mixture of three different gases.

If the total pressure of the mixture is 1.55 atm, calculate the partial pressure of the yellow gas.

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