Question

A 20.0 liter cylinder containing a mixture of oxygen and
nitrogen gas is sitting at room temperature (25.0 ^{o}C).
Given that the mole fraction of nitrogen is 0.24, and the partial
pressure of oxygen is 1.60 atm, what is the total pressure of the
gas mixture in this container?

Answer #1

Given that the mole fraction of nitrogen is 0.24

Then, mole fraction of oxygen = 1- 0.24 = 0.76 [ sum of mole fraction of all the species = 1]

Also given that partial pressure of oxygen = 1.60 atm

We know that

Partial pressure of gas = mole fraction of the gas x total pressure of the gas mixture

Then,

Partial pressure of oxygen = mole fraction of oxygen x total pressure of the gas mixture

1.6 atm = 0.76 x total pressure of the gas mixture

Then,

total pressure of the gas mixture = 1.6 atm/ 0.76 = 2.105 atm

Therefore,

the total pressure of the gas mixture in the container = 2.105 atm

A gas mixture containing 80 mole% nitrogen and the balance
n-hexane flows through a pipe at a rate of 90 m3/h. The gauge
pressure is 1 atm and the temperature is 95 oC.
a) Is the gas saturated or superheated? Find its degrees of
superheat assuming this operation runs at constant pressure.
b) To what temperature would the gas have to be cooled at
constant pressure in order to condense 80% of the hexane?

1. A gas mixture containing oxygen, nitrogen, and helium exerts
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Exercise 11.76
A mixture of helium, nitrogen, and oxygen has a total pressure
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Part A
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Part B
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