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We are asked to calculate the number of moles of CCl_{3}F in the gas phase.

Use the ideal gas law :

$\overline{){\mathbf{PV}}{\mathbf{}}{\mathbf{=}}{\mathbf{}}{\mathbf{nRT}}}\phantom{\rule{0ex}{0ex}}\mathbf{n}\mathbf{}\mathbf{=}\mathbf{}\frac{\mathbf{PV}}{\mathbf{RT}}\mathbf{}$

Convert the values need to be consistent with R.

R = 0.08206 L-atm/mol-K

$\mathrm{P}=856\overline{)\mathbf{torr}}\mathbf{}\times \frac{1\mathrm{atm}}{760\overline{)\mathbf{torr}}\mathbf{}}=1.12\mathrm{atm}$

V = 1.2 L

T = 300 K

The vapor pressure of CCl_{3}F at 300 K is 856 torr. If 12.5 g of CCl_{3} F is enclosed in a 1.2 L container, calculate the number of moles of CCl_{3}F in the gas phase.

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

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Based on our data, we think this problem is relevant for Professor Scott's class at OLE MISS.