Question

A helium balloon is launched in the atmosphere. If the balloons volume is 4.19 x 10^3 liters at 22.5 C and the atmosphereic pressure is 754 mm Hg, What will be the balloons volume at a height of 20 miles where the pressure is 76 mm Hg and the temperature is -33 C. Hint: use the ideal gas law at constant number of moles

Answer 1

Ideal gas constant

PV = nRT

R = nT/PV

volume = 4.19 10³

temparature = 22.5⁰c

pressure = 754 mmhg

R = nT/PV

   = 1 22.5   = 0.000006   

7544.1910³

PV = nRT

V=nRT / P

   = 1 0.000006 33

   76

= 0.000002 (Or) 2 10⁵ liters.