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Answer:
The total air pressure at the top of the highest peak in the world is 253.5 torr
Explanation:
The partial pressures of the gases present at the top of Mount Everest are;
Nitrogen, N₂ = 201.0 torr
Oxygen, O₂ = 50.0 torr
Argon, Ar = 2.0 torr
Carbon dioxide, CO₂ = 0.5 torr
By Dalton's law of partial pressure, the total pressure that a mixture of gases exerts is equal to the sum of the partial pressures of the individual gases
Mathematically, the law can be expressed as follows;
Total pressure, P = ∑P[tex]_i[/tex] = P₁ + P₂ + · · ·
From which we have;
The total air pressure at the top of the highest peak in the world, Mount Everest, [tex]P_{Total Mont Everest}[/tex] = The sum of the partial pressures of N₂, O₂, Ar, and CO₂
[tex]P_{Total Mont Everest}[/tex] = 201.0 torr + 50.0 torr + 2.0 torr + 0.5 torr = 253.5 torr
[tex]P_{Total Mont Everest}[/tex] = 253.5 torr = 0.33355263 atmosphere
Therefore, the total air pressure at the top of the highest peak in the world, [tex]P_{Total Mont Everest}[/tex] = 253.5 torr
The total air pressure at the top of the highest peak in the world is 253.5 torr.
What is Dalton's Law?
Dalton's law of gases states that total pressure of any mixture of gases is equal to the sum of the partial pressures of individual gases.
Given that,
Partial pressure of Nitrogen gas = 201 torr
Partial pressure of Oxygen gas = 50 torr
Partial pressure of Argon gas = 2 torr
Partial pressure of Carbon dioxide gas = 0.5 torr
Total pressure at the top = 201 + 50 + 2 + 0.5 = 253.5 torr
Hence total pressure is 253.5 torr.
To know more about partial pressure, visit the below link:
https://brainly.com/question/19813237
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