A container consisting mixture of 28 ~g ~N ₂, 8 ~g~ He and 40 g Ne at 25^ C . If the total pressure exerted by the gaseous mixture is 20 bar, What is the partial pressure exerted by N ₂ ?

Step-by-step solution

Partial pressure of N₂ Using Dalton’s Law: P_ N₂ = X_ N₂ P_ total . Molar masses: N₂ = 28~ g/mol , He = 4~ g/mol , Ne = 20~ g/mol . Moles: n_ N₂ = 28/28 = 1 , n_ He = 8/4 = 2 , n_ Ne = 40/20 = 2 . Total moles: n_ total = 1 + 2 + 2 = 5 . Mole fraction X_ N₂ = 1/5 = 0.2 . Substitute: P_ N₂ = 0.2 20 = 4~ bar . The partial pressure of nitrogen is 4~ bar .