Amixture of n2, o2 and he have mole fractions of 0.25, 0.65, and 0.10, respectively. what is the pressure of n2 if the total pressure of the mixture is 3.9 atm?

The pressure of nitrogen in the mixture has been 0.975 atm.

Partial pressure has been defined as the pressure exerted by the gas molecules in the mixture. The partial pressure ()  has been expressed as:

Where,  Mole fraction of the element A,

The total pressure of the mixture,

Substituting the values, the pressure of nitrogen (),

The pressure of nitrogen in the mixture has been 0.975 atm.

For more information about mole fraction, refer to the link:

link

Partia pressure N₂ → 0.975 atm

Explanation:

Let's analyse the moles fractions:

N₂ → 0.25

O₂ → 0.65

He → 0.1

Partial pressure / Total pressure = Mole fraction

Partial pressure N₂ / 3.9 atm = Mole fraction N₂

Partial pressure N₂ / 3.9 atm = 0.25

Partial pressure N₂ = 3.9 atm . 0.25 → 0.975 atm

the ideal gas law equation is as follows

pv = nrt

where p - pressure

v - volume

n - number of moles

r - universal gas constant

t - temperature

so if the pressure, volume and temperature are already known

we are left with n and r

since r is the universal gas constant that has a known fixed value then r too is known

so we are left with 'n'

once we know temperature volume and pressure

we can find the number of moles of gas present using the ideal gas law equation

this is not my own answer, this is an answer for the same question by the user blahblahmali. i do not claim ownership of this account.

catya your not at all which answer i've seen you do this on another question!