Question

A sample of gas occupies a volume of 725 ml at 825 torr. at constant temperature, what will be the new pressure when the volume changes to the following:

(a) 359 ml


(b) 4.94 l


torr

Answer 1

Okay, let's break this down step-by-step:

* We are given:

- Initial volume: 725 ml

- Initial pressure: 825 torr

- Temperature is constant

* The key relationship we can use is Boyle's Law:

P1V1 = P2V2

Where:

P1 = initial pressure

V1 = initial volume

P2 = final pressure (what we want to calculate)

V2 = final volume

* For part (a), the final volume is 359 ml. Plugging into Boyle's Law:

825 torr * 725 ml = P2 * 359 ml

P2 = (825 torr * 725 ml) / 359 ml = 1698 torr

The new pressure will be 1698 torr when the volume changes to 359 ml.

* For part (b), the final volume is 4.94 L. Converting to ml, that is 4940 ml. Plugging into Boyle's Law:

825 torr * 725 ml = P2 * 4940 ml

P2 = (825 torr * 725 ml) / 4940 ml = 207 torr

The new pressure will be 207 torr when the volume changes to 4.94 L (4940 ml).

So in summary:

(a) When volume changes to 359 ml, new pressure is 1698 torr

(b) When volume changes to 4.94 L (4940 ml), new pressure is 207 torr