What will be the volume of the balloon?

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SUMMARY

The volume of a helium balloon at an altitude of 22 miles, with initial conditions of 1400L at 0.950 atm and 18°C, is calculated using the gas law equation (P1V1)/T1 = (P2V2)/T2. After converting 4 Torr to 0.005 atm, the final volume V2 is determined to be approximately 25,1374 L. The significant increase in volume is attributed to the low pressure at high altitude, confirming the calculations are correct despite initial doubts about the result.

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[SOLVED] Gas Law Problem

Homework Statement


An expandable balloon contains 1400L of He at 0.950 atm pressure and 18 deg C. At an altitude of 22 miles (temp 2 deg C, and pressure 4 Torr. What will be the volume of the balloon?


Homework Equations


(P1V1)/T1 = (P2V2)/T2
1 atm = 760 Torr
K = 273 + Deg C

The Attempt at a Solution


First thing I did was to convert Torr to atm, so 4 Torr = .005 atm.
I then solved for V2 so I get the equation :
V2 = (T2P1V1)/(T2P2) or (275k(0.95atm)1400L)/(291k(.005atm))= 25,1374 L

My Answer seems way off as it is so huge. Where did I make a mistake?
Thanks
 
Last edited:
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your calculations are correct, its the low pressure that is making it so big
 
Thanks. It just looked off to me, glad you clarified for me. That would have to be one stretchy balloon though :)
 

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