Agas mixture contains 1.20 g n2 and 0.77 g o2 in a 1.65-l container at 15 ∘c. part a calculate the mole fraction of n2. express your answer using two significant figures. x1 x 1 = nothing request answer part b calculate the mole fraction of o2. express your answer using two significant figures. x2 x 2 = nothing request answer part c calculate the partial pressure of n2. express your answer using two significant figures. p1 p 1 = nothing atm request answer part d calculate the partial pressure of o2. express your answer using two significant figures. p2 p 2 = nothing atm request answer provide feedback

Explanation:

Moles of nitrogen gas =

Moles of oxygen gas =

Mole fraction of nitrogen gas=

Mole fraction of oxygen gas=

Total  umber of moles in container :

n == 0.0428 mol + 0.0240 mol = 0.0668 mol

Volume of the container = V = 1.65 L

Temperature of the container = T = 15°C = 288.15 K

Total pressure in the container = P

Using an ideal gas equation:

P = 0.9577 atm

Partial pressure of nitrogen gas =

Partial pressure of nitrogen gas =

Partial pressure of nitrogen gas and oxygen gas can be calculated by using Dalton's law of partial pressure:

frequency, z, and the collision density, z, in carbon dioxide (co2), r 180 pm at 30 °c and 120 kpa

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