Question

56g of nitrogen and 96 g of oxygen are mixed isothermally and the mixture exerts a total pressure of 10 atm. The partial pressure of nitrogen and oxygen are respectively

Answer 1

Concept : According to Dalton's law of partial pressure

Partial pressure = Total pressure × mole fraction

Explanation :

Moles of nitrogen $n_{N_{2} } = \frac{56}{28} = 2$

Moles of oxygen $n_{O_{2} } = \frac{96}{32} =  3$

Moles fraction of oxygen $x_{o_{2} } = \frac{3}{3+2} =   0.6$

Mole fraction of nitrogen $x_{n_{2} } = \frac{2}{2+3} =   0.4$

Given that,

Total pressure = 10 atm

Therefore,

Partial pressure of nitrogen $p_{n_{2} } = 10*0.4 = 4 atm$

Partial pressure of oxygen $p_{o_{2} } = 10*0.6 = 6 atm$

Answer 2

plz check the answer in the attached photo