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:

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.

it forms an anion that has a larger radius. anions have a negative charge and are larger than the original atom.