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?

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