Academic Subjects
➤
Chemistry
➤
General Chemistry
➤
Gases
➤
Calculating Volume Of 0.023 Mole "Dry" Hydrogen At STP
If a metal reacts with a strong acid at
25 ℃
and produces
0.023 mole
of H
2
,
what is the volume of "dry" hydrogen at S
T
P
?
To find the volume of dry hydrogen at STP, we want to apply the Ideal Gas Law
p
V
=
n
R
T
where R = 0.082057
L
atm
mol
-1
K
-1
Let's take a quick look at what STP means
Standard Temperature (0 °C = 32 °F = 273.15 K)
&
Standard Pressure (1 atm)
dry hydrogen means pure hydrogen, i.e. hydrogen only
25 °C is the T at which this metal reacts with acid,
i.e. useless info for solving this problem
And we're ready to fill in our values
(1
atm
)(
V
) = (0.023
moles
)
(0.082057
L
atm
)
/
mole
K
(273.15
K
)
(1
atm
)(
V
) = (0.5155189
L
atm
)
(
V
) =
(0.5155189
L
atm
)
/
(1
atm
)
(
V
) = 0.5155189
L
The volume of dry H
2
at STP is 5.2 x 10
-1
L