A gas-filled balloon having a volume of 3.50 L at 1.2 atm and 25°C is allowed to rise to the stratosphere (about 30 km above the surface of Earth), where the temperature and pressure are −23°C and 3.00 10−3 atm, respectively. Calculate the final volume of the balloon.

(P1V1)/T1 = (P2V2)/T2

250 To solve this problem, we can use the combined gas law, which relates the initial and final conditions of pressure, volume, and temperature.

The combined gas law equation is:
(P1 × V1) / (T1) = (P2 × V2) / (T2)

Given values:
P1 = 1.2 atm (initial pressure)
V1 = 3.50 L (initial volume)
T1 = 25°C = 298 K (initial temperature)
P2 = 3.00 * 10^(-3) atm (final pressure)
T2 = -23°C = 250 K (final temperature)

Let's plug in the values and solve for V2 (final volume):
(1.2 atm × 3.50 L) / (298 K) = (3.00 × 10^(-3) atm × V2) / (250 K)

Now, solve for V2:
(1.2 atm × 3.50 L × 250 K) / (298 K) = 3.00 × 10^(-3) atm × V2

V2 = (1.2 atm × 3.50 L × 250 K) / (298 K × 3.00 × 10^(-3) atm)

Using the above equation, we can calculate the final volume of the balloon.