Answer:
Explanation:
P
V
=
n
R
T
where:
P
=
pressure
V
=
volume
n
=
moles
R
=
universal constant
(
8.314
k
P
a
⋅
L
m
o
l
⋅
K
)
T
=
temperature (Kelvin)
Recall that at STP conditions:
P
=
101.325
k
P
a
T
=
273.15
K
To solve for the number of moles of carbon dioxide gas, substitute your known values into the ideal gas equation:
P
V
=
n
R
T
n
=
P
V
R
T
n
=
(
101.325
k
P
a
)
(
5.6
L
)
(
8.314
k
P
a
⋅
L
m
o
l
⋅
K
)
(
273.15
K
)
n
=
(
101.325
k
P
a
)
(
5.6
L
)
(
8.314
k
P
a
⋅
L
m
o
l
⋅
K
)
(
273.15
K
)
n
=
0.2498580892
m
o
l
n
=
0.25
m
o
l
(rounded to
2
significant figures)
