A gas-filled weather balloon with a volume of 51.5 L is released at sea-level conditions of 755 torr and 23°C.

Question

A gas-filled weather balloon with a volume of 51.5 L is released at sea-level conditions of 755 torr and 23°C. The balloon can expand to a maximum volume of 760. L. When the balloon rises to an altitude at which the temperature is -5°C and the pressure is 0.059 atm, what will be the final volume of balloon?

Answer 1

Please use the ideal gas law.
PV/T = pv/t
755*51.5/296 = (0.059*760)*v/268
v = 755*51.5*268/(296*0.059*760) = 785 (L)
So the weather balloon bursts and final volume of balloon is undefined.

Answer 2

okay this is very simple. for this question you are solving for V2 = volume 2 or final volume. 835L is not the final volume you will be solving for, thats the maximum volume that the balloon can hold okay. initial condtions: Volume = 55.0 L Pressure = 755 torr or 0.9934 atm temperature = 23 degrees celcius or 296.15 kelvin final conditions: Volume = ? pressure = 0.066 atm temperature = -5 degrees celcius or 268.15 kelvin remember the question is asking you if at the final conditions is the volume of the balloon at the max or not. okay and you will simply just use the general gas equation (P1 * V1) / t1 = (P2 * V2) / t2 >>> where 1 refers to the initial conditions and 2 refers to the final conditions and P = pressure, V = volume and t = temperature. okay so now all you have to do is isolate for V2 and that would be... V2 = (P1 * V1 * t2) / (t1 * P2) = (0.9934atm)(55.0L)(268.15k) / (296.15k)(0.066atm) = ANSWER!! sorry i dont have a calculator on me, but this is correct because if you do the unit analysis ( see which units cancel out) you are left with L which is the unit for volume!. so anyways if the volume is 835L then yes it will reach its maximum volume at the final conditions and if its not 835L then no.