Academic Subjects
➤
Chemistry
➤
General Chemistry
➤
Gases
➤
Calculating Moles Of Gas To Fill An Average Man’s Lungs
How many moles of gas would it take to fill an average man’s lungs,
total capacity of which is about
4.5 L
? Assume
1 atm
pressure and
37 ℃
A. 11.2 mol
B. 0.75 mol
C. 37 mol
D. 1.24 mol
E. 0.177 mol
Applying the Ideal Gas Law, we first want to check if all units match
R 0.082057
L
atm
mol
-1
K
-1
We will have to convert our temperature value
37.00 °C
+ 273.15 =
310.15 K
Now, we're ready for
p
V
=
n
R
T
(1
atm
)(4.5
L
) = (
x
)
(0.082057
L
atm
)
/
mole
K
(310.15
K
)
(4.5
L
) = (
x
)
(25.45
L
)
/
mole
(
x
) =
(4.5
L
)
/
(25.45
L
mole
-1
)
x
= 0.1768
moles
An average man's lungs will hold 0.177 moles of gas
Answer E is the correct option