Problem: A sample of 3.10 g of SO2 (g) originally in a 5.20-L vessel at 26 oC is transferred to a 12.0-L vessel at 25 oC. A sample of 2.40 g N2 (g) originally in a 2.60-L vessel at 20 oC is transferred to this same 12.0-L vessel.What is the partial pressure of N2 (g) in this vessel?

FREE Expert Solution

We’re being asked to calculate for the partial pressure of N2 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:

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

Problem Details

A sample of 3.10 g of SO2 (g) originally in a 5.20-L vessel at 26 oC is transferred to a 12.0-L vessel at 25 oC. A sample of 2.40 g N2 (g) originally in a 2.60-L vessel at 20 oC is transferred to this same 12.0-L vessel.

What is the partial pressure of N2 (g) in this vessel?