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What is the pressure of a mixture of nitrogen (N2) and oxygen (O2) if partial pressure of N2 is 594 mm Hg and the partial pressure of O2 is 165 mm Hg?

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Neetoo

Answer:

Total pressure = 759 mmHg

Explanation:

Given data:

Partial pressure of oxygen = 165 mmHg

Partial pressure of nitrogen = 594 mmHg

Total pressure = ?

Solution:

According to Dalton law of partial pressure,

The total pressure inside container is equal to the sum of partial pressures of individual gases present in container.

Mathematical expression:

P(total) = P₁ + P₂ + P₃+ ............+Pₙ

Total pressure = P(O₂) +  P(N₂)

Total pressure =  165 mmHg + 594 mmHg

Total pressure = 759 mmHg

Eduard22sly

The pressure of the mixture containing nitrogen and oxygen is 759 mmHg

From the question given above, the following data were obtained:

Partial pressure of N₂ = 594 mmHg

Partial pressure of O₂ = 165 mm Hg

Pressure of mixture =?

The pressure of the mixture can be obtained by using the Dalton's law partial pressure as follow:

Total pressure = Partial pressure of N₂ + Partial pressure of O₂

Total pressure = 594 + 165

Total pressure = 759 mmHg

Therefore, the pressure of the mixture is 759 mmHg

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