Answer:
[tex]\large \boxed{\text{1.14 atm}}[/tex]
Explanation:
The identity of the gases doesn't matter. All we need is the total number of moles.
1. Total number of moles
N₂ 0.0388 mol
CO 0.147
H₂ 0.0802
0.266 mol
2. Other data
V = 5.73 L
T = 25 °C
3. Total pressure
We can use the Ideal Gas Law:
pV = nRT
Calculations:
(a) Convert the temperature to kelvins
T = (25 + 273.15) K = 298.15 K
(b) Calculate the pressure
[tex]\begin{array}{rcl}pV & =& nRT\\p \times \text{5.73 L} & = & \text{0.266 mol} \times \text{0.082 06 L$\cdot$ atm$\cdot$K$^{-1}$mol$^{-1}\times$ 298.15 K}\\5.73p & = & \text{6.361 atm}\\p & = & \textbf{1.14 atm}\end{array}\\\text{The total pressure in the flask is $\large \boxed{\textbf{1.14 atm}}$}[/tex]
