A gas is placed in a container with a moveable piston. It is then cooled down at constant pressure. What happens? Explain.
1 answer:
Answer:
The piston will move down
Explanation:
We can solve this problem by using Charle's Law, which states that:
"For a fixed mass of an ideal gas kept at constant pressure, the volume of the gas is directly proportional to the absolute temperature of the gas"
Mathematically:
where
V is the volume of the gas
T is the absolute temperature of the gas
In this problem, we have a gas placed in a container with a moveable piston. We are also told that the gas is kept at constant pressure, so we can apply Charle's Law.
We are told that the gas is cooled down: this means that its absolute temperature decreases. Therefore, according to Charle's Law, this means that the volume of the gas also decreases: therefore, the piston of the container will move down.
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The total pressure of the mixture is 65.5 kPa.
According to Dalton's Law of Partial Pressure,
The partial pressure of gas = Mole fraction of gas × Total pressure
Total Pressure = Sum of all the gases partial pressures
The number of moles of methane is,
= 0.021 mols
The moles of methane are 0.021 mols.
The number of moles of the argon,
= 0.003 mols
The number of moles of argon is 0.003 mols.
The number of moles of nitrogen is,
= 0.010 mols
The number of moles of nitrogen is 0.010 mols.
The total number of moles is,
= 0.021 + 0.003 + 0.010
= 0.034 mols
= 0.29
= 65.5 kPa
Therefore, the total pressure of the mixture is 65.5 kPa.
To know more about Dalton's law, refer to the below link:
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