Asealed container has 1 mole of helium and 2 moles of nitrogen at 30dc when the total pressure of mixture is 0.60 atm what is the partial pressure of the nitrogen?

The partial pressure of  nitrogen is  0.402 atm.

Explanation:

Given data:

Number of moles of helium = 1 mol

Number of moles of nitrogen = 2 mol

Total pressure of mixture = 0.60 atm

Partial pressure of nitrogen = ?

Solution:

First of all we will calculate the mole fraction of nitrogen.

mole fraction of nitrogen = moles of nitrogen / total number of moles

mole fraction of nitrogen = 2 mol / 3 mol = 0.67

Partial pressure of nitrogen:

P₁ = [ n₁ /n(t)] × Pt

P₁ = 0.67 × 0.60 atm

P₁ = 0.402 atm

it means there are 3 atoms of oxygen