A 2.0 liter balloon at a temperature of 25°C contains 0.1 mol of oxygen and 0.4 mol of nitrogen, what is the partial pressure of nitrogen?

Aug 8, 2016

Approx. $5 \cdot a t m$ with respect to ${N}_{2}$.

Explanation:

Dalton's law of partial pressures states that in a gaseous mixture, the pressure exerted by a component is the same as the pressure it would exert if it ALONE ooccupied the container. The total pressure, is the sum of the partial pressures.

So given this, I merely have to solve the Ideal Gas equation:

P_"dinitrogen"=(n_"nitrogen"*R*T)/(V) $=$ $\frac{0.4 \cdot \cancel{m o l} \times 0.0821 \cdot \cancel{L} \cdot a t m \cdot \cancel{{K}^{-} 1} \cdot \cancel{m o {l}^{-} 1} \times 298 \cdot \cancel{K}}{2 \cdot \cancel{L}}$

I get an answer in $a t m$, as required.