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

V₂ = 1518L

Step-by-step explanation:

-Using combined gas law:

`(P_1V_1)/(T_1) =(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:

`(743torr*975L)/(303.15K) =(375torrV_2)/(238.15K)`

V₂ = 1518L