The pressure in the flask is 3.4 atm.
pV = nRT
T = (20 + 273.15) K = 293.15 K
p = (nRT)/V = (1.4 mol × 0.082 06 L·atm·K⁻¹mol⁻¹ × 293.15 K)/10 L = 3.4 atm
Explanation:
The given data is as follows.
P = ?, V = 10 liter
n = 1.4 moles, T = [tex]20^{o}C[/tex] = (20 + 273) K = 293 K
As per the ideal gas equation, PV = nRT. Therefore, putting the given values into the formula as follows.
PV = nRT
[tex]P \times 10 L = 1.4 mol \times 0.0821 Latm/mol K \times 293 K[/tex]
P = 3.36 atm
= 3.4 atm (approx)
Thus, we can conclude that the pressure in the flask in units of atmospheres is 3.4 atm.
