Answer to Question #181472 in Chemistry for fff

Question

A balloon has a volume of 4.0 L when at sea level (1.0 atm) at a room temperature of

28 °C. What will be its volume when inflated with the same amount of gas at an elevation

where the atmospheric pressure is 200 mm Hg at 28°C?

Answer 1

Solution:

Convert atm to mmHg:

(1 atm) × (760 mmHg / 1 atm) = 760 mmHg

P₁ = 1 atm = 760 mmHg

V₁ = 4.0 L

T₁ = T₂ = 28°C = const

P₂ = 200 mmHg

V₂ = unknown

Since the temperature and amount of gas remain unchanged, Boyle's law can be used.

Boyle's gas law can be expressed as: P₁V₁ = P₂V₂

To find the volume, solve the equation for V₂:

V₂ = P₁V₁ / P₂

V₂ = (760 mmHg × 4.0 L) / (200 mmHg) = 15.2 L

V₂ = 15.2 L

 

Answer: The volume will be 15.2 L.