Question

g at constant temperature, a sample of helium at 2 atm in a closed container was compressed from 5.00 L to 3.00 L. what was the new pressure exerted by the helium on its container

Answer 1

The new pressure exerted by helium on its container is 2533.33 torr.

Boyle's law: For a fixed amount of an ideal gas kept at a fixed temperature, pressure and volume are inversely proportional. so PV= constant.

At constant temperature and moles,

P1V1 = P2V2.

The original sample is at 2atm torr and volume 5.00 L and then helium gas was compressed to 3.00 L

∴ P₁V₁ = P₂V₂

 (2× 760 torr)(5.00 L ) = (3.00 L )(x torr),

 x = 2533.33 torr.

 P₂ = 2533.33 torr.

Therefore, the new pressure exerted by helium on its container is 2533.33 torr.

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