Calculate number of moles of 560ml hydrogen gas at STP.
Answers
Explanation:
The molar mass (molecular mass in grams) is
45 g
.
Explanation:
Note: This is going to be a long answer.
First determine the number of moles.
STP=273.15 K and 100 kPa
Use the ideal gas law.
P
V
=
n
R
T
,
where
P
is pressure in kiloPascals
(
kPa
)
,
V
is volume in liters
(
L
)
,
n
is moles,
R
is the gas constant, and
T
is temperature in Kelvins
(
K
)
.
Given/Known
P
=
100 kPa
T
=
273.15 K
V
=
560
mL
×
1
L
1000
mL
=
0.56 L
R
=
8.3144598 L kPa K
−
1
mol
−
1
Unknown
moles, n
Equation
P
V
=
n
R
T
Solution
Rearrange the equation to isolate
n
and solve.
n
=
P
V
R
T
=
n
=
(
100
kPa
)
(
0.56
L
)
(
8.3144598
L
kPa
K
−
1
mol
−
1
)
=
0.024658 mol
n
=0.024658 mol
(keeping a couple of guard digits)
Determine the molecular (molar) mass.
Given/Known
n
=0.024658 mol
m
=
mass
=
1.10 g
Unknown
Molar mass:
MM
Equation
n
=
m
MM
Solution
Rearrange the equation to isolate
MM
and solve.
MM
×
m
n
MM
×
1.10
g
0.024658
mol
=
MM
=
45 g/mol
(rounded to two significant figures due to 0.56 L)
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