A Baloon is filled with 3.00 L of helium at a pressure of 765 Torr. What is the volume of the baloon at an altitude where the atmospheric pressure is 530 torr?
use P1V1=P2V2
To determine the volume of the balloon at an altitude where the atmospheric pressure is 530 torr, we can use Boyle's Law. Boyle's Law states that the volume of a gas is inversely proportional to its pressure at constant temperature.
The formula for Boyle's Law is:
P1 * V1 = P2 * V2
Where:
P1 = initial pressure (765 torr)
V1 = initial volume (3.00 L)
P2 = final pressure (530 torr)
V2 = final volume (unknown)
Rearranging the formula, we can solve for V2:
V2 = (P1 * V1) / P2
Plugging in the values:
V2 = (765 torr * 3.00 L) / 530 torr
Now we can calculate the volume of the balloon at an altitude with atmospheric pressure of 530 torr:
V2 = 4.34 L
Therefore, the volume of the balloon at an altitude where the atmospheric pressure is 530 torr is approximately 4.34 L.