Your SlideShare is downloading. ×
12.2
Upcoming SlideShare
Loading in...5
×

Thanks for flagging this SlideShare!

Oops! An error has occurred.

×

Introducing the official SlideShare app

Stunning, full-screen experience for iPhone and Android

Text the download link to your phone

Standard text messaging rates apply

12.2

152
views

Published on

Published in: Education

0 Comments
0 Likes
Statistics
Notes
  • Be the first to comment

  • Be the first to like this

No Downloads
Views
Total Views
152
On Slideshare
0
From Embeds
0
Number of Embeds
0
Actions
Shares
0
Downloads
0
Comments
0
Likes
0
Embeds 0
No embeds

Report content
Flagged as inappropriate Flag as inappropriate
Flag as inappropriate

Select your reason for flagging this presentation as inappropriate.

Cancel
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's 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
  • 6. Avogadro's Law
    • 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.