The pressure of a sample of helium is 2.0 atm in a 200-ml container. if the container is compressed to 100 ml without changing the temperature, what is the new pressure?

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Answer 1

The new pressure of the helium sample is 4.0 atm. When the volume of the container is reduced from 200 ml to 100 ml while keeping the temperature constant, according to Boyle's Law,

the product of pressure and volume remains constant. Therefore, since the initial pressure is 2.0 atm and the initial volume is 200 ml, the new pressure can be calculated by the equation P1V1 = P2V2, where P1 and V1 are the initial pressure and volume, and P2 and V2 are the final pressure and volume. Plugging in the values, we get (2.0 atm)(200 ml) = (P2)(100 ml). Solving for P2, we find P2 = 4.0 atm. Thus, the new pressure is 4.0 atm after compressing the container.

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