A weather balloon is inflated to a volume of 28.6 L at a pressure of 737 mmHg and a temperature of 26.8 ∘C. The balloon rises in the atmosphere to an altitude where the pressure is 385 mmHg and the temperature is -16.3 ∘C. Assuming the balloon can freely expand, calculate the volume of the balloon at this altitude.

Volume of the balloon at this altitude is 46.9 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 = 737 mm Hg

= final pressure of gas =  385 mm Hg

= initial volume of gas = 28.6 L

= final volume of gas = ?

= initial temperature of gas =

= final temperature of gas =

Now put all the given values in the above equation, we get:

Thus the volume of the balloon at this altitude is 46.9 L

i think 4.44 moles

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