# What is the total pressure in a 6.00-L flask which contains 0.127 mol of H_2 (g) and 0.288 mol of N_2 (g) at 20.0°C?

Jun 14, 2016

Approx. $1.7 \cdot a t m$

#### Explanation:

The pressures are additive by Dalton's Law of Partial Pressures: the pressure exerted by a gas in a gaseous mixture is the same as the pressure it would exert if it alone occupied the container. I could calculate the individual partial pressures, or simply calculate the pressure based on the COMBINED molar quantities:

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

$\frac{0.415 \cdot \cancel{m o l} \times 0.0821 \cdot \cancel{L} \cdot a t m \cdot \cancel{{K}^{-} 1} \cdot \cancel{m o {l}^{-} 1} \times 293 \cdot \cancel{K}}{6.00 \cdot \cancel{L}}$
$\cong$ ??*atm

Given what I have said, can you calculate the partial pressures, ${P}_{\text{dihydrogen}}$, and ${P}_{\text{dinitrogen}}$?