Question

A high-altitude balloon is filled with 1.41 x 104 L of hydrogen at a temperature of 21 °C and a pressure of 745 torr. What is the volume of the balloon at a height of 20 km, where the temperature is -48 °C and the pressure is 63.1 torr

Answer 1

Answer:

1.27 x 10⁵ L

Explanation:

V₁ = initial volume = 14100 L

V₂ = final volume = ?

P₁ = initial pressure = 745 torr

P₂ = final pressure = 63.1 torr

T₁ = initial temperature = 21 °C = 21 + 273 = 294 K

T₂ = final temperature = - 48 °C = - 48 + 273 = 225 K

Using the equation

$\frac{P_{1}V_{1}}{T_{1}} = \frac{P_{2}V_{2}}{T_{2}}$

$\frac{(745)(14100)}{294} = \frac{(63.1)V_{2}}{225}$

$V_{2}$ = 1.27 x 10⁵ L