Question

A 200.0 liter container of nitrogen gas has a pressure 6250 torr. If the container was compressed until its volume become exactly half of what it was, what is the pressure inside the container now in torr?

Answer 1

The pressure inside the container after compression is 12,500 torr.

Step-by-step explanation:

To find the pressure inside the container after it is compressed to half its volume, we can use Boyle's Law, which states that the pressure and volume of a gas are inversely proportional when temperature is constant. Initially, the volume of the container is 200.0 L and the pressure is 6250 torr. When the volume becomes half, it becomes 100.0 L. To find the final pressure, we can use the equation: P1 x V1 = P2 x V2, where P1 and V1 are the initial pressure and volume, and P2 and V2 are the final pressure and volume.

Using the equation:

6250 torr x 200.0 L = P2 x 100.0 L

P2 = (6250 torr x 200.0 L) / 100.0 L = 12,500 torr

Therefore, the pressure inside the container after compression is 12,500 torr.