Question

A mixture of He He , N 2 N2 , and Ar Ar has a pressure of 24.1 24.1 atm at 28.0 28.0 °C. If the partial pressure of He He is 3013 3013 torr and that of Ar Ar is 2737 2737 mm Hg, what is the partial pressure of N 2 N2

Answer 1

16.5 atm

Step-by-step explanation:

A mixture of He, N₂, and Ar has a pressure of 24.1 atm at 28.0 °C. If the partial pressure of He is 3013 torr and that of Ar is 2737 mm Hg, what is the partial pressure of N₂?

The total pressure of a gaseous mixture is equal to the sum of the partial pressures.

P = pHe + pN₂ + pAr

pN₂ = P - pHe - pAr [1]

We need to express pHe and pAr in atm.

`pHe=3013torr.(1atm)/(760torr) =3.96atm`

`pAr=2737mmHg.(1atm)/(760mmHg) =3.60atm`

From [1],

pN₂ = 24.1 atm - 3.96 atm - 3.60 atm = 16.5 atm