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:$76.21\times 10^4 L$

Explanation:

Given

$P_{initial}=752\ mm\ of\ Hg$

$T_{initial}=27.8^{\circ}\approx 300.8 K$

$V_{initial}=9.47\times 10^4 L$

$P_{final}=73 mm\ of\ Hg$

$T_{final}=235 K$

use PV=nRT

$\frac{PV}{T}=constant$

$\frac{P_{initial}\times V_{initial}}{T_{initial}}=\frac{P_{final}\times V_{final}}{T_{final}}$

$\frac{752\times 9.47\times 10^4}{300.8}=\frac{73\times V}{235}$

$V=76.21 \times 10^4 L$