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