A weather balloon is inflated to a volume of 27.6 L at a pressure of 755 mmHg and a temperature of 29.9 ∘C. The balloon rises in the atmosphere to an altitude where the pressure is 385 mmHg and the temperature is -14.1 ∘C. Assuming the balloon can freely expand, calculate the volume of the balloon at this altitude.

The volume of the balloon at this altitude is 46.3 L

Explanation:

Combined gas law is the combination of Boyle's law, Charles's law and Gay-Lussac's law

The combined gas equation is,

where,

= initial pressure of gas = 755 mm Hg

= final pressure of gas (at STP) = 385 mm Hg

= initial volume of gas = 27.6 L

= final volume of gas = ?

= initial temperature of gas =

= final temperature of gas =

Putting all the values we get:

Thus the volume of the balloon at this altitude is 46.3 L

away from the curb

explanation:

the wheels would then hit the curb if it started to rolling, decreasing the chance of an accident.