At constant temperature, a sample of helium at 760. torr in a closed container was compressed from 5.00 l to 3.00 l, with no change in moles or temperature. what was the new pressure exerted by the helium on its container?

Question

Chemistry

Berlynn

30 September, 04:18

At constant temperature, a sample of helium at 760. torr in a closed container was compressed from 5.00 l to 3.00 l, with no change in moles or temperature. what was the new pressure exerted by the helium on its container?

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Answers (1)

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Whispy · Answer 1

To solve this problem, we will use Boyle's law which states that:

At constant temperature, P1V1 = P2V2 where:

P1 is the initial pressure = 760 torr

V1 is the initial volume = 5 liters

P2 is the final pressure that we want to calculate

V2 is the final volume = 3 liters

Substitute in the above equation to get P2 as follows:

(760) (5) = P2 (3)

P2 = (760*5) / (3) = 1266.667 torr