Question

A mixture of He

, N2
, and Ar
has a pressure of 13.6
atm at 28.0
°C. If the partial pressure of He
is 1831
torr and that of Ar
is 997
mm Hg, what is the partial pressure of N2
?

Answer 1

Answer : The partial pressure of nitrogen gas in the mixture is, 9.88 atm

Explanation :

According to the Dalton's Law, the total pressure of the gas is equal to the sum of the partial pressure of individual gases.

Formula used :

`p_T=p_(He)+p_(Ar)+p_(N_2)`

where,

`p_T` = total pressure of gas = 13.6 atm

`p_(He)` = partial pressure of helium gas = 1831 torr = 2.41 atm

`p_(Ar)` = partial pressure of argon gas = 997 torr = 1.31 atm

Conversion used: (1 atm = 760 torr)

`p_(N_2)` = partial pressure of nitrogen gas = ?

Now put all the given values in the above formula, we get:

`13.6=2.41+1.31+p_(N_2)`

`p_(N_2)=9.88atm`

Thus, the partial pressure of nitrogen gas in the mixture is, 9.88 atm