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How many air molecules are in a 13.0×12.0×10.0 ft room (28.2 L=1 ft3)? Assume atmospheric pressure of 1.00 atm, a room temperature of 20.0 ∘C, and ideal behavior.

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opudodennis

Answer:

1963.93 Moles

Explanation:

-We know the standard conversion ratio for the volume of a mole is [tex]1 Mole=22.4L[/tex]

Given volume of rooms as [tex]13.0ft\times12.0ft\times10ft=1560 ft^3[/tex]

Convert the volume into liters:[tex]1560\times28.2l=43992l[/tex]

#From our conversion ratio above, we get the volume of air molecules in moles as:

[tex]V_m=\frac{43992L}{22.4L}\times 1\ mole\\\\=1963.93\ Moles[/tex]

Hence, the volume of air molecules is 1963.93 Moles