Question

A helium-filled balloon is launched when the temperature at ground level is 27.8°C and the barometer reads 752 mmHg. If the balloon's volume at launch is 9.47 × 10 4 4 L, what is the volume in Liters at a height of 36 km, where the pressure is 73.0 mm Hg and temperature is 235.0 K?

Answer 1

Answer:
`76.21* 10^4 L`

Step-by-step explanation:

Given

`P_(initial)=752\ mm\ of\ Hg`

`T_(initial)=27.8^(\circ)\approx 300.8 K`

`V_(initial)=9.47* 10^4 L`

`P_(final)=73 mm\ of\ Hg`

`T_(final)=235 K`

use PV=nRT

`(PV)/(T)=constant`

`(P_(initial)* V_(initial))/(T_(initial))=(P_(final)* V_(final))/(T_(final))`

`(752* 9.47* 10^4)/(300.8)=(73* V)/(235)`

`V=76.21 * 10^4 L`