$\overline{){\mathbf{PV}}{\mathbf{=}}{\mathbf{nRT}}}\phantom{\rule{0ex}{0ex}}\phantom{\rule{0ex}{0ex}}\mathbf{n}\mathbf{=}\frac{\mathbf{m}}{\mathbf{M}}\phantom{\rule{0ex}{0ex}}\phantom{\rule{0ex}{0ex}}(\mathrm{PV}=\frac{m}{\overline{)M}}\mathrm{RT})\overline{)\left(M\right)}\phantom{\rule{0ex}{0ex}}\phantom{\rule{0ex}{0ex}}\frac{\mathbf{PVM}}{\mathbf{RT}}\mathbf{=}\frac{\mathbf{m}\overline{)\mathbf{RT}}}{\overline{)\mathbf{RT}}}\phantom{\rule{0ex}{0ex}}\phantom{\rule{0ex}{0ex}}\overline{){\mathbf{m}}{\mathbf{=}}\frac{\mathbf{PVM}}{\mathbf{RT}}}$

A gas mixture contains each of the following gases at the indicated partial pressures: N_{2}, 221 torr ; O_{2}, 131 torr ; and He, 131 torr .

What mass of each gas is present in a 1.30 -L sample of this mixture at 25.0 ^{o}C?

Frequently Asked Questions

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 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.