1 / 5

50 likes | 310 Vues

Charles Law V 1 = V 2 P constant T 1 T 2 Boyles Law P 1 V 1 = P 2 V 2 T constant Combined P 1 V 1 = P 2 V 2 T 1 T 2 Gay-Lussac’s Law P 1 = P 2 V constant T 1 T 2.

Télécharger la présentation
## Charles Law V 1 = V 2 P constant T 1 T 2

**An Image/Link below is provided (as is) to download presentation**
Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author.
Content is provided to you AS IS for your information and personal use only.
Download presentation by click this link.
While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server.
During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

**Charles Law V1 =V2 P constant**T1 T2 Boyles Law P1V1 = P2V2 T constant Combined P1V1=P2V2 T1 T2 Gay-Lussac’s Law P1=P2 V constant T1 T2 ALL temperatures must be in Kelvin!!**Ideal Gas Equation**PV=nRT P pressure V volume (L) n moles T temperature (K) R gas constant .082 L∙atm mol∙K 8.31 L∙kPa mol∙K 62.4 L∙torr mol∙K**Find Volume**What volume would be occupied by 1.00 moles of gas at 0˚C and 1 atm pressure? V= nRT=(1.00 mole)(.082 L∙atm/mol∙K)(273K) P 1 atm = 22.4L**When given three of the four variables, we can find the**fourth. A gas has a volume of 2.20L at 25◦C. If there are .085 moles of the gas, under what pressure must the gas be held? P = nRT V P = (.085mole)(0.0821 L∙atm)(298K) 2.20L mol∙K = .945 atm (or 95.8 kPa or 718 torr)**Find moles**A gas has a volume of 31.2L at 28˚C and 82.6 kPa. How many moles are in the sample? n = PV = (82.6kPa)(31.2L) RT (8.31kPa∙L/mol∙K)(301K) = 1.03 mol How many molecules would that be? 1.03 mol x 6.02 x 1023 molecules/mol = 6.20 x 1023 molecules

More Related