Question

A 975 L balloon contains helium. On the ground the temperature is 30 0C and the pressure is 743 torr. What will be the balloon's volume at an altitude of 5700 m where the pressure is 375 mm Hg and the temperature is -35.0 0C?

Answer 1

Answer:

V₂ = 1518L

Explanation:

-Using combined gas law:

$\frac{P_1V_1}{T_1} =\frac{P_2V_2}{T_2}$

Where P is pressure, V is volume and T is absolute temperature of 1, initial state and 2, final state of the gas.

Initial states:

P₁ = 743 torr

V₁ = 975L

T₁ = 30°C + 273.15K = 303.15K

P₂ = 375 mmHg = torr

V₂ = Our incognite

T₂ = -35°C + 273.15K = 238.15K

Replacing:

$\frac{743torr*975L}{303.15K} =\frac{375torrV_2}{238.15K}$

V₂ = 1518L