Question

A 32.0 L cylinder containing helium gas at a pressure of 38.5 atm is used to fill a weather balloon in order to lift equipment into the stratosphere. What is the final pressure (in atm) in the cylinder after a 355 L balloon is filled to a pressure of 1.20 atm.

Answer 1

Step-by-step explanation:

We can use Boyle's Law, which states that the product of pressure and volume is constant for a fixed amount of gas at a constant temperature. We can use this law to find the final pressure in the cylinder after filling the balloon.

The initial pressure and volume of the helium gas in the cylinder are:

P1 = 38.5 atm

V1 = 32.0 L

The final volume of the gas after filling the balloon is:

V2 = 355 L

Using Boyle's Law, we can write:

P1V1 = P2V2

where P2 is the final pressure in the cylinder.

Solving for P2, we get:

P2 = (P1V1) / V2

Plugging in the values, we get:

P2 = (38.5 atm x 32.0 L) / 355 L

P2 = 3.48 atm

Therefore, the final pressure in the cylinder after filling the balloon is 3.48 atm.