30moles of CO2 and 60 moles of N² are mixed in a vessell at 25⁰c the total pressures of the mixture is 180 mm of the Hg what are the partical pressurly of co² and
Answers
Answer:
explosion is here
Explanation:
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A mixture of gases contains 0.75 mol N2, 0.30 mol O2, and 0.15 mol CO2. If the total pressure of the mixture is 1.56 atm, what is the partial pressure of each component?
Chemistry Partial Pressure
1 Answer
Stefan V.
Dec 22, 2015
Here's what I got.
Explanation:
To make this problem a little interesting, let's assume that you're not familiar with Dalton's Law of partial pressures, which tells you that the partial pressure of a gas that's part of a gaseous mixture is proportional to that gas' mole fraction.
Here's how you can think about what's going on, Let's assume that the mixture is at a pressure
P
total
, a temperature
T
, and occupies a volume
V
.
If you were to isolate the nitrogen gas in the same volume, you could write, using the ideal gas law equation
P
N
2
⋅
V
=
n
N
2
⋅
R
T
⇒
P
N
2
=
n
N
2
⋅
R
T
V
Here
P
N
2
is the pressure exerted by the nitrogen gas when alone in the same volume as the mixture.
Now do the same for oxygen and carbon dioxide.
P
O
2
⋅
V
=
n
O
2
⋅
R
T
⇒
P
O
2
=
n
O
2
⋅
R
T
V
P
C
O
2
⋅
V
=
n
C
O
2
⋅
R
T
⇒
P
C
O
2
=
n
C
O
2
⋅
R
T
V
Now, what would happen if you were to have the nitrogen gas, the oxygen gas, and the carbon dioxide in the same volume? The pressure would change to
P
total
, and the total number of moles in the mixture would be
n
total
=
n
N
2
+
n
O
2
+
n
C
O
2
This means that you could write
P
total
⋅
V
=
n
total
⋅
R
T
P
total
=
n
total
⋅
R
T
V
This is equivalent to
P
total
=
[
n
N
2
+
n
O
2
+
n
C
O
2
]
⋅
R
T
V
(
1
)
P
total
=
P
N
2
n
N
2
⋅
R
T
V
+
P
O
2
n
O
2
⋅
R
T
V
+
P
C
O
2
n
C
O
2
⋅
R
T
V
Therefore,
P
total
=
P
N
2
+
P
O
2
+
P
C
O
2