A 25 l partially filled weather balloon has a volume of 11 L at sea level where the pressure is 1 atm. It rises to an altitude of 6.096km (20,000 feet) where the pressure is only .48 atm. What is the resulting volume? At what pressure would it burst? Use the internet to find this altitude ___km.

To find the resulting volume of the weather balloon at an altitude of 6.096 km, we can use Boyle's Law, which states that the pressure and volume of a gas are inversely proportional when temperature remains constant.

Boyle's Law formula:
P1 × V1 = P2 × V2

Given:
P1 (pressure at sea level) = 1 atm
V1 (initial volume) = 25 L
P2 (pressure at 6.096 km) = 0.48 atm
V2 (resulting volume) = ?

Using the formula, we can plug in the given values and solve for V2:

1 atm × 25 L = 0.48 atm × V2

25 = 0.48V2

V2 = 25 / 0.48

V2 ≈ 52.08 L

Therefore, the resulting volume of the weather balloon at an altitude of 6.096 km is approximately 52.08 liters.

To find the altitude at which the balloon would burst, we need to know the maximum volume it can reach before bursting. This depends on the material and structural integrity of the balloon. Without that information, it is challenging to provide an exact answer. However, typically, weather balloons burst when the volume has expanded to a certain point where the pressure inside the balloon becomes greater than the external pressure.

As for finding the altitude in km corresponding to a pressure of 0.48 atm, we can use the Barometric Formula. However, it requires knowledge of the temperature profile of the atmosphere, which is beyond the scope of the internet search capability of this AI.