Question

A sealed balloon is filled with 1.00L of Helium at 23 C and at a pressure of 4.45atm . The balloon rises to a point in the atmosphere where the pressure is 0.289 atm and the temperature is - 31 C . What is the new volume , in liters ?

Answer 1

We can use the combined gas law to solve this problem:

(P1V1)/T1 = (P2V2)/T2

where P1, V1, and T1 are the initial pressure, volume, and temperature, respectively, and P2 and T2 are the final pressure and temperature, respectively. We can solve for V2, the final volume:

V2 = (P1V1T2)/(P2T1)

Plugging in the values we have:

V2 = (4.45 atm * 1.00 L * 242 K) / (0.289 atm * 296 K)

V2 = 132.5 L

Therefore, the new volume of the balloon is approximately 132.5 liters.

Step-by-step explanation: