# 0.250*mol quantities of dinitrogen and sulfur dioxide are enclosed in a 2.5*L vessel at a temperature of 300*K. What are the partial pressures of each gas, and what is the total pressure?

May 10, 2017

$\text{We use Dalton's Law of Partial Pressures...........}$ to get ${P}_{\text{Total}} = 5 \cdot a t m$

#### Explanation:

In a gaseous mixture, the partial pressure exerted by a gaseous component is the same as the pressure it would exert if it ALONE occupied the container. The total pressure is the sum of the individual partial pressures.

And thus we simply use the Ideal Gas Law:

$P = \frac{n R T}{V}$

${P}_{S {O}_{2}} = \frac{0.25 \cdot m o l \times 0.0821 \cdot \frac{L \cdot a t m}{K \cdot m o l} \times 300 \cdot K}{2.5 \cdot L}$

$= 2.5 \cdot a t m$

And likewise, ${P}_{{N}_{2}} = {P}_{S {O}_{2}} = 2.5 \cdot a t m$

P_"Total"=P_(SO_2)+P_(N_2)=??*atm.