A helium balloon with an internal pressure of 1.0 atm and a volume of 4.50 L at 20.0⁰C is released. What volume will the balloon occupy at an altitude where the pressure is 60.78 kPa and the temperature is -20.0⁰C?

Volume occupied by volume is 6.48 L at an altitude where the pressure is 60.78 kPa and the temperature is -20.0⁰C

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 = 1 atm = 101.3 kPa

= final pressure of gas = 60.78 kPa

= initial volume of gas =  4.50 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:

The volume occupied by volume is 6.48 L at an altitude where the pressure is 60.78 kPa and the temperature is -20.0⁰C

2b2t

explanation:

2b2t

it is a solid

explanation: