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An open flask sitting in a lab refrigerator looks empty, but it is actually filled with a mixture of gases called air. If the flask volume is 2.00 L, and the air is at standard temperature and pressure, how many gaseous molecules does the flask contain?

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Respuesta :

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.

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