Question

An expandable balloon filled with 100.0 l of helium at 750 torr and 20����c is launched from ground level. No gas is added or removed from the balloon during its flight. Calculate its volume at an altitude of 10 km, where the temperature and pressure in the balloon is 2.0����c and 190 torr, respectively. Show work.

Answer 1

The volume of the balloon at an altitude of 10 km is approximately 90.68 L.

Step-by-step explanation:

To calculate the volume of the balloon at an altitude of 10 km, we can use the combined gas law equation:

P1V1/T1 = P2V2/T2

First, we need to convert the temperatures from Celsius to Kelvin by adding 273.15:

T1 = 20 + 273.15 = 293.15 K

T2 = 2 + 273.15 = 275.15 K

Then, we can plug in the values into the equation:

(750 torr)(100.0 L)/(293.15 K) = (190 torr)(V2)/(275.15 K)

Solving for V2:

V2 = (750 torr)(100.0 L)(275.15 K)/(190 torr)(293.15 K) ≈ 90.68 L