Respuesta :
Explanation:
According to ideal gas equation, product of pressure and volume equals the product of number of moles, gas constant and temperature.
Mathematically, PV = nRT
where P = pressure, V = volume
n = no. of moles, R = gas constant = 0.0821 atm L/mol
T = temperature
Since, it is known that number of moles equal mass divided by molar mass.
Hence, number of moles of given sample of acetone are as follows.
No. of moles = [tex]\frac{mass}{\text{molar mass of acetone}}[/tex]
= [tex]\frac{6.06 \times 10^{-2}}{58 g/mol}[/tex]
= [tex]0.104 \times 10^{-2}[/tex] mole
Therefore, putting the values in ideal gas equation as follows.
PV = nRT
[tex]P \times 0.36 L = 0.104 \times 10^{-2} \times 0.082 atm L/mol \times 281 K[/tex]
= 0.359 atm
In 1 atm equal to 760 mm Hg. So, convert 0.359 atm into mm Hg as follows.
[tex]0.359 atm \times \frac{760 mm Hg}{1 atm}[/tex]
= 272.84 mm Hg
Hence, pressure of the ideal gas will be 100 mm Hg + 272.84 mm Hg = 372.84 mm Hg
Thus, we can conclude that the ideal gas pressure in the container if all of the liquid acetone evaporated is 372.84 mm Hg.
