p1 x V1 = p2 x V2
so
p1 = [1.0 (atm) x 6.25 (L)] / 2.875 (L) = 2.17 atm
1875 mL
1.75 atm
well at 100 ft you are at about 4 atmospheres pressure, so a gas would have about 1/4th the volume it did on the surface.
This problem can be solved with the ideal gas law. The original pressure and volume of the container are proportional the final pressure and volume of the container. The original pressure was 1 atmosphere and the original volume was 1 liter. If the final volume is 1.8 liters, then the final pressure is 0.55 atmospheres.
the answer is 72.1 Hg
You don't. Liters is a unit of volume, atmospheres is a unit of pressure.
Atmospheres cannot be converter to milliliters. Atmospheres are a unit of pressure based on the Earth's atmosphere. Milliliters are a unit of volume, otherwise known as a cubic centimeter.
The pressure is 172,84 atmospheres.
1875 mL
If the temperature of the gas is decreasing, then in order to maintain constant pressure, you would have to compress it in volume.
1.75 atm
I do not believe you can compress a gas without any heat being generated to the environment.
of Compress, Pressed together; compacted; reduced in volume by pressure., Flattened lengthwise.
At standard temperature and pressure, it will...if you heat the gas or compress it, it will have a different volume.
The big reason is because air is air, and water is water. The second reason is because air is compressible, while water cannot be compressed. What that means is that if you compress air to twice the pressure, it will be one-half the volume. If you compress water to be twice the pressure, the volume won't change.
well at 100 ft you are at about 4 atmospheres pressure, so a gas would have about 1/4th the volume it did on the surface.
atmospheres