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A gas has an initial pressure of 633 torr and an initial volume of 87.3 mL. What is its new pressure if volume is changed to 45.0 mL?

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Answer:

1230 torr

Explanation:

To solve this problem, all you need to do is apply Boyle's Gas Law: P1V1 = P2V2.

633 torr x 87.3 mL = 45.0 mL x P2 (Unknown)

P2 = 1230 torr

(Remember, we need to follow sig fig rules.)

The statement of the new pressure is "1228.02"

What is a pressure?

The physical force exerted on an item is known as pressure. The pressure and volume of the gas are maintained at a constant temperature according to Boyle's law, that is pressure and volume are inversely proportional.

P1.V1 = P2.V2

Now,

P1 = 633 torr and V1 = 87.3 mL

V2 = 45.0 mL

In order to find the new volume, substituting these values into Boyle’s law, we get

[tex]P2\;=\;\frac{P1.V1}{V2} \\P2\;=\;\frac{(633\; torr).(87.3\;mL)}{(45.0\;mL)} \\[/tex]

P2 = 1228.02 torr

Hence the correct answer is 1228.02 torr.

Learn more about pressure here

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