0
Upcoming SlideShare
×

Thanks for flagging this SlideShare!

Oops! An error has occurred.

×
Saving this for later? Get the SlideShare app to save on your phone or tablet. Read anywhere, anytime – even offline.
Standard text messaging rates apply

# 12.2

199

Published on

0 Likes
Statistics
Notes
• Full Name
Comment goes here.

Are you sure you want to Yes No
• Be the first to comment

• Be the first to like this

Views
Total Views
199
On Slideshare
0
From Embeds
0
Number of Embeds
0
Actions
Shares
0
0
0
Likes
0
Embeds 0
No embeds

No notes for slide

### Transcript

• 1. Gas Laws 12.2
• 2. Variables you need to know
• P = pressure exerted by the gas
• V = volume of the gas
• T = temperature in Kelvin
• n = number of moles of gas
• (Oh yes, you will need mole island.)
• 3. Boyle’s Law
• Deals with pressure and volume .
• As pressure increases, volume decreases. The opposite is also true.
• P 1 V 1 =P 2 V 2
• See page 425 for example
• 4. Charles' Law
• Deals with temperature and volume .
• An increase in temperature will cause an increase in volume. The opposite is also true.
• V 1 /T 1 = V 2 /T 2
• See page 428 for example
• 5. Gay-Lussac’s Law
• Deals with pressure and temperature .
• Increased temperature = increased pressure. The opposite is also true.
• P 1 /T 1 = P 2 /T 2
• See page 430 for example
• Gas volume is directly proportional to the number of moles of gas at the same temperature and pressure.
• The problem is volume changes with temperature and pressure.
• STP 0 0 C and 1 atmosphere
• V 1 /n 1 =V 2 /n 2
• You will have to use mole island to convert volume (Liters) & moles.
• 7. Homework
• P.425 1-3
• P.428 1-3
• P.431 1-3
• There is an example of how to do each problem in the book.
• Show all work.
• Round to the 100 th .