Question

A helium balloon with an internal pressure of 1.25 atm and a volume of 3.50 L at 25.00 C

is released. What volume will the balloon occupy at an altitude where the pressure is
0.800 atm and the temperature is -30.00 C?

Answer 1

Using the combined gas law ((P1•V1)/T1) = ((P2•V2)/T2), you get ((1.25atm•3.5L)/298K) = ((0.800atm•V2)/243K). Solving for V2 you get 4.46L.