Answer :
Considering the Dalton's law, the pressure of the pure oxygen is 736.2 torr.
Dalton's law
The pressure exerted by a particular gas in a mixture is known as partial pressure.
So, Dalton's law states that the total pressure of a gas mixture is equal to the sum of the pressures that each gas would exert if it were alone:
[tex]P_{T} =P_{1} +P_{2} +...+P_{n}[/tex]
where n is the amount of gases present in the gas mixture.
This relationship is due to the assumption that there are no attractive forces between the gases.
Pressure of the pure oxygen
In this case, you know that there is a mixture of oxygen gas and gaseous water (steam). Then the total pressure of a gas mixture is
[tex]P_{T} =P_{O_{2} } +P_{water}[/tex]
You know:
- the total pressure of the gas mixture is [tex]P_{T} =[/tex]760 Torr.
- the pressure of gaseous water is [tex]P_{water} =[/tex]23. 8 torr.
Replacing:
[tex]760 torr=P_{O_{2} } +23.8 torr[/tex]
Solving:
[tex]P_{O_{2} } =760 torr - 23.8 torr[/tex]
[tex]P_{O_{2} } =[/tex]736.2 torr
Finally, the pressure of the pure oxygen is 736.2 torr.
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Final answer:
To find the pressure of the pure oxygen in a gas mixture collected over water, subtract the pressure of the water vapor from the total pressure.
Explanation:
When collecting a sample of oxygen over water, the total pressure of the gas mixture is a combination of the pressure of oxygen and gaseous water (steam). To find the pressure of the pure oxygen, we need to subtract the pressure of the water vapor from the total pressure. In this case, the pressure of gaseous water is given as 23.8 torr. Therefore, the pressure of the pure oxygen is 760 torr - 23.8 torr = 736.2 torr.
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