Considering the Dalton's partial pressure, the partial pressure of nitrogen in the tank is 41 atm.
The pressure exerted by a particular gas in a mixture is known as its 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_{3} + ... +P_{n}[/tex]
where n is the amount of gases present in the mixture.
This relationship is due to the assumption that there are no attractive forces between the gases.
In summary, the total pressure in a mixture of gases is equal to the sum of partial pressures of each gas.
In this case, the total pressure of the gas mixture is calculated as:
[tex]P_{T} =P_{oxygen} +P_{helium} +P_{nitrogen}[/tex]
You know that:
Replacing in the expression for the total pressure:
[tex]180 atm=81 atm+58 atm+P_{nitrogen}[/tex]
Solving:
180 atm -81 atm -58 atm= [tex]P_{nitrogen}[/tex]
41 atm= [tex]P_{nitrogen}[/tex]
Finally, the partial pressure of nitrogen in the tank is 41 atm.
Learn more about Dalton's partial pressure:
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