We’re being asked to **calculate the partial pressure of SO**_{2} in a **12.0 L flask **at **25 °C**.

We will use **ideal gas equation** to calculate for the pressure:

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

P = pressure, atm

V = volume, L

n = moles, mol

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

T = temperature, K

**But first, we have to ****calculate the amount of SO _{2} in moles.**

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 SO_{2} (g) in the larger container?

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