Status: Not yet answered | Points possible: 1.00 A sample of chlorine gas starting at 681 mm Hg is placed under a pressure of 992 mm Hg and reduced to a volume of 543.8 mL.
What was the initial volume, in ml, of the chlorine gas container if the process was performed at constant temperature?
Type

V1 = 792.1 ml

Explanation:

The product of pressure and volume is constant when temperature is constant. This relationship is known as Boyle's law.

To answer this, I assume the chlorine gas will behave as a perfect gas. In reality this is not completely true.

P1*V1 = P2*V2

Given:

P1 = 681 mm Hg

V1 = ?

P2 = 992 mm Hg

V2 = 543.8 ml

V1 = ( P2 * V2 ) / P1

V1 = (992 *543.8 ) / 681

V1 = 792.143318649046 ml

V1 = 792.1 ml

sorry i was late, but i don't know what assignment your talking about, i'm in flvs as well, im in earth space science. but u are behind pace bc every class should be in the 3's or 4'