Question

A gas mixture contains 1.25 g N2 and 0.84 g O2 in a 1.53-L container at 14 ∘C.

A.) Calculate the mole fraction of N2.

B.) Calculate the mole fraction of O2.

C.) Calculate the partial pressure of N2.

D.) Calculate the partial pressure of O2.

Answer 1

As we know the number of moles can be found by the rule

n= number of moles

w= given mass

M= molar mass

For N₂, the number of moles is

For O₂, the number of moles is

Total number of mole

A) mole fraction of N₂ that means ,  which can be determined by

B)

mole fraction of O₂ that means ,  which can be determined by

C) partial pressure can be calculated by using Ideal gas equation

here volume = 1.53 L

R= gas constant,

Now apply

P₁ is the partial pressure of N₂

D) Apply above equation to find out the partial pressure of O₂, which is denoted as P₂

here volume = 1.53 L

R= gas constant,

Now apply

Hence the partial pressure for O₂ is 0.39atm