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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
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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?

User Byroncorrales
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3.9k points

1 Answer

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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.
User Seshu Vinay
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4.3k points
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