equal masses of He and H2 are present in a container the mole fraction of he is what
Answers
Answer:
Explanation:
The idea here is that the partial pressure of hydrogen gas will depend on
the mole fraction of hydrogen gas in the mixture
the total pressure of the mixture
Now, let's say that we are mixing
m
g
of hydrogen gas and
m
g
of methane.
Use the molar masses of the two gases to express the number of moles of each component of the mixture in terms of their mass
m
m
g
⋅
1 mole H
2
2.0
g
=
(
m
2
)
moles H
2
m
g
⋅
1 mole CH
4
16.0
g
=
(
m
16
)
moles O
2
The total number of moles of gas present in the mixture will be equal to
(
m
2
)
.
moles
+
(
m
16
)
.
moles
=
(
9
16
⋅
m
)
.
moles
Now, the mole fraction of hydrogen gas is calculated by dividing the number of moles of hydrogen gas by the total number of moles of gas present in the mixture.
χ
H
2
=
(
m
2
)
moles
(
9
16
⋅
m
)
moles
=
1
2
⋅
16
9
=
8
9
By definition, the partial pressure of hydrogen gas in the mixture is equal to
P
H
2
=
χ
H
2
⋅
P
total
In your case, this will be equal to
P
H
2
=
8
9
⋅
P
total