We use ideal gas equation,
[tex]PV=nRT[/tex] ,
[tex]V=\frac{nRT}{P}[/tex] or [tex]V= (\frac{m}{M}) \frac{RT}{P}[/tex]
Here, V is the volume, P is pressure and T is temperature and [tex]n=\frac{m}{M}[/tex] , m is the mass and M is the molar mass and R is universal gas constant its value of 8.3144621 L kPa/K mol
Given, [tex]P = 90 \ kPa[/tex] , [tex]T = 27 ^0C = (27 +273) = 300 \ k[/tex] and [tex]m = 4.40 \ g[/tex].
The molar mass of the carbon dioxide, [tex]M = 44.010 \ g/mol[/tex] .
Substituting these values in above equation, we get
[tex]V = (\frac{4.40 \ g}{44.010 \ g/mol })\frac{8.3144621 L kPa/K mol \times300 \ K }{90 \ kPa} \\\\ V = 2.77 L[/tex].
Thus, the volume of the flask is 2.77 L.
The volume of the gas is 2.76 L.
We have the following information;
pressure = 90 kpa or 0.89 atm
temperature = 27 celcius or 300 K
number of moles = 4.40 g/44 g/mol = 0.1 moles
volume = ?
Now;
Using PV = nRT
V = nRT/P
V = 0.1 moles × 0.082 atmLK-1mol-1 × 300 K/ 0.89 atm
V = 2.76 L
The volume of the gas is 2.76 L.
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