Question

A sealed 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?

Answer 1

Answer:

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