Answer: [tex]67.4\times 10^{23}[/tex] molecules are there in the flask
Explanation:
According to the ideal gas equation:
[tex]PV=nRT[/tex]
P = Pressure of the gas = 1 atm
V= Volume of the gas = 2.00 L
T= Temperature of the gas = 273 K [tex]0^00C=273K[/tex]
R= Gas constant = 0.0821 atmL/K mol
n= moles of gas
[tex]n=\frac{RT}{PV}=\frac{0.0821\times 273}{1\times 2.00}=11.2[/tex]
According to avogadro's law, 1 mole of every substance occupies 22.4 L at STP and contains avogadro's number [tex]6.023\times 10^{23}[/tex] of particles.
1 mole of gaseous air contains = [tex]6.023\times 10^{23}[/tex] molecules
11.2 moles of gaseous air contains = [tex]\frac{6.023\times 10^{23}}{1}\times 11.2=67.4\times 10^{23}[/tex] molecules
[tex]67.4\times 10^{23}[/tex] gaseous molecules are contained in the flask.
