Gas Laws Question ... 10 pts!?

  • Thread starter Thread starter <3twilight
  • Start date Start date
3

<3twilight

Guest
A balloon with a maximum volume of 1.50 L is filled 2/3 full with helium at sea level and released into the atmosphere. If the initial pressure was 1.00 atm and the pressure drops 90.0 torr per 1000 M in altitude, how high will the balloon be when it pops assuming no temperature change.

Please show work and explain. Thank you!
 
From what I can tell... And I'm a little rusty but

1 ATM = 760 torr.

760 torr / 1.50 times the original pressure = 507 torr. This should be the maximum the balloon can take. It should be at 1.5L at that point.

760 torr - 507 torr = 253 torr. The difference between sea level and the maximum capacity.

253 torr / 90.0 torr/km = 2.81 km before the balloon bursts.

Please double check my thinking and significant figure math. As I said, I'm a little rusty.
 
Back
Top