Question

DO NOT TROLL AND ANSWER WITHOUT THE CORRECT ANSWER! I EXPECT THE CORRECT ANSWER NOT A TROLL SO IF YOU DONT HAVE THE ANSWER DO NOT WRITE ANYTHING. IF YOU TROLL I WILL REPORT YOU

A weather balloon with a volume of 3.40774 L

is released from Earth’s surface at sea level.

What volume will the balloon occupy at an

altitude of 20.0 km, where the air pressure is

10 kPa?

Answer in units of L.

Answer 1

Answer:  The volume occupied at an altitude of 20.0 km is 34.5289 L

Explanation:

Boyle's Law: This law states that pressure is inversely proportional to the volume of the gas at constant temperature and number of moles.

$P\propto \frac{1}{V}$     (At constant temperature and number of moles)

where,

$P_1$ = initial pressure of gas = 101.325 kPa ( sea level)

$P_2$ = final pressure of gas = 10 kPa

$V_1$ = initial volume of gas = 3.40774 L

$V_2$ = final volume of gas = ?

Now put all the given values in the above equation, we get the final pressure of gas.

$101.325\times 3.40774=10\times V_2$

$V_2=34.5289L$

Therefore, the volume occupied at an altitude of 20.0 km is 34.5289 L