Question

A mixture of He , N 2 , and Ar has a pressure of 16.7 atm at 28.0 °C. If the partial pressure of He is 1737 torr and that of Ar is 2087 mm Hg, what is the partial pressure of N 2 ?

Answer 1

The answer to your question is P N₂ = 11.67 atm

Step-by-step explanation:

Data

He 1737 torr

N₂ = ?

Ar 2087 mmHG

Total pressure = 16.7 atm

Process

1.- Convert torr to atm

1 atm --------------- 760 torr

x -------------- 1737 torr

x = (1737 x 1)/760

x = 2.29 atm

2.- Convert mmHg to atm

1 atm ----------------- 760 mmHg

x ---------------- 2087 mmHG

x = (2087 x 1)/760

x = 2.74

3.- Find the Partial pressure of N₂

Total pressure = He pressure + N₂ pressure + Ar pressure

- Substitution

16.7 = 2.29 + P N₂ + 2.74

- Solve for P N₂

P N₂ = 16.7 - 2.29 - 2.74

P N₂ = 11.67 atm