We’re being asked to calculate for the partial pressure of N_{2} in a 12.00-L container.

We’re going to calculate the pressure of a gas using the **ideal gas equation**:

$\overline{){\mathbf{PV}}{\mathbf{=}}{\mathbf{nRT}}}$

P = pressure, atm

V = volume, L

n = moles, mol

R = gas constant = 0.08206 (L·atm)/(mol·K)

T = temperature, K

*Rearranging the ideal gas equation:*

$\frac{\mathbf{P}\overline{)\mathbf{V}}}{\overline{)\mathbf{V}}}\mathbf{=}\frac{\mathbf{nRT}}{\mathbf{V}}\phantom{\rule{0ex}{0ex}}\overline{){\mathbf{P}}{\mathbf{=}}\frac{\mathbf{nRT}}{\mathbf{V}}}$

A sample of 3.10 g of SO_{2} (g) originally in a 5.20-L vessel at 26 ^{o}C is transferred to a 12.0-L vessel at 25 ^{o}C. A sample of 2.40 g N_{2} (g) originally in a 2.60-L vessel at 20 ^{o}C is transferred to this same 12.0-L vessel.

What is the partial pressure of N_{2} (g) in this vessel?

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.