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A 3.00 L cylinder at 25 degrees Celsius contains a mixture of 3 gases: He, N2, and Ar at partial pressures of 115, 285, and 325 torr, respectively. If all the He is removed from the mixture and the temperature does not change, what will be the partial pressure, in torr, of the N2

Respuesta :

Answer:

[tex]P_{N_2}=285 torr[/tex]

Explanation:

Given that

Volume of cylinder = 3 L

Temperature= 25 degrees

Partial pressure of the gases

[tex]P_{He}=115 torr[/tex]

[tex]P_{N_2}=285 torr[/tex]

[tex]P_{Ar}=325 torr[/tex]

By using Dalton's law , the total pressure of the non reacting gas is the sum of the partial pressure of all gases.

[tex]P_{total}=P_{He}+P_{N_2}+P_{Ar}[/tex]

[tex]P_{total}=115+285+325=725 torr[/tex]

When all the He gas will removed then partial pressure of He will be zero.

[tex]P_{total}=P_P_{N_2}+P_{Ar}[/tex]

[tex]P_{total}=285+325=610 torr[/tex]

Partial pressure of N₂

[tex]P_{N_2}=610-325=285 torr[/tex]

[tex]P_{N_2}=285 torr[/tex]

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