The pressure of a mixture within a rigid container of nitrogen, carbon dioxide and oxygen is 150 kPa. What is the partial pressure of oxygen if the partial pressures of nitrogen and carbon dioxide are 100 kPa and 24
kPa, respectively?

P(O₂) = 26KPa

Explanation:

Given data:

Total pressure = 150 KPa

Partial pressure of nitrogen = 100 KPa

Partial pressure of carbon dioxide = 24 KPa

Partial pressure of oxygen = ?

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

Now we will solve this  problem by using this law.

P (total) = P(O₂) + P(N₂) + P(CO₂)

150 KPa =   P(O₂) + 100 KPa + 24 KPa

150 KPa = P(O₂) + 124 KPa

P(O₂) = 150 KPa  - 124 KPa

P(O₂) = 26KPa