Question

A 17.0 L helium tank is pressurized to 22.0 atm. When connected to this tank, a balloon will inflate because the pressure inside the tank is greater than the atmospheric pressure pushing on the outside of the balloon. Assuming the balloon could expand indefinitely and never burst, the pressure would eventually equalize causing the balloon to stop inflating. What would the volume of the balloon be when this happens? Assume atmospheric pressure is 1.00 atm. Also assume ideal behavior and constant temperature. volume: 374 L

Answer 1

Answer:

The volume of the balloon would be 374 L.

Explanation:

Initially, He occuplies a volume of 17.0 L (V₁) at a pressure of 22.0 atm (P₁). If pressure decreases to 1.00 atm (P₂), volume is expected to increase. Assuming ideal behavior of the gas and constant temperature, we can calculate the final volume (V₂) using Boyle's Law.

$P_{1} \times V_{1} = P_{2} \times V_{2}\\V_{2} = \frac{P_{1} \times V_{1}}{P_{2}} =\frac{22.0atm \times 17.0L}{1.00atm} = 374 L$