Question

An apparatus consists of a 4.0 dm3 flask containing nitrogen gas at 25 oC and 803 kPa. It is joined by a valve to a 10.0 dm3 flask containing argon gas 25 oC and 47.2 kPa. The valve is opened and the gases mix. i. What is the partial pressure of each gas after mixing?

Answer 1

Partial pressure of nitrogen = 229.43 kpa

Partial pressure of argon = 33.7 Kpa

Step-by-step explanation:

Given data:

Volume of flask one = 4.0 dm³

Temperature = 25°C

Pressure of nitrogen = 803 KPa

Final volume = 4.0 dm³ + 10.0 dm³ = 14.0 dm³

Initial volume of argon = 47.2 KPa

Final pressure of both gases when valve is open = ?

Solution:

For nitrogen:

P₁V₁ = P₂V₂

803 KPa × 4 dm³ = P₂ × 14.0 dm³

P₂ = 803 KPa × 4 dm³ / 14.0 dm³

P₂ = 3212 kpa / 14.0

P₂ = 229.43 kpa

For argon:

P₁V₁ = P₂V₂

47.2 KPa × 10.0 dm³ = P₂× 14.0 dm³

P₂ = 47.2 KPa × 10.0 dm³/14.0 dm³

P₂ = 472 kpa/ 14.0

P₂ = 33.7 Kpa