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Observe yourself breathing and count the number of times you inhale per second. During each breath you probably inhale 0.66 L of air. Assume the pressure is 1 atm and the temperature is 20∘C. Only about 21% of air is O2. 1. How many oxygen molecules do you inhale if you are at sea level?

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To solve this exercise it is necessary to apply the concepts related to Robert Boyle's law where:

[tex]PV=nRT[/tex]

Where,

P = Pressure

V = Volume

T = Temperature

n = amount of substance

R = Ideal gas constant

We start by calculating the volume of inhaled O_2 for it:

[tex]V = 21\% * 0.66L[/tex]

[tex]V = 0.1386L[/tex]

Our values are given as

P = 1atm

T=293K [tex]R = 0.083145kJ*mol^{-1}K^{-1}[/tex]

Using the equation to find n, we have:

[tex]PV=nRT[/tex]

[tex]n = \frac{PV}{RT}[/tex]

[tex]n = \frac{(1)(0.1386)}{(0.0821)(293)}[/tex]

[tex]n = 5.761*10^{-3}mol[/tex]

Number of molecules would be found through Avogadro number, then

[tex]\#Molecules = 5.761*10^{-3}*6.022*10^{23}[/tex]

[tex]\#Molecules = 3.469*10^{21} molecules[/tex]

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