• Save
12.2
Upcoming SlideShare
Loading in...5
×
 

12.2

on

  • 284 views

 

Statistics

Views

Total Views
284
Views on SlideShare
284
Embed Views
0

Actions

Likes
0
Downloads
0
Comments
0

0 Embeds 0

No embeds

Accessibility

Categories

Upload Details

Uploaded via as Microsoft PowerPoint

Usage Rights

© All Rights Reserved

Report content

Flagged as inappropriate Flag as inappropriate
Flag as inappropriate

Select your reason for flagging this presentation as inappropriate.

Cancel
  • Full Name Full Name Comment goes here.
    Are you sure you want to
    Your message goes here
    Processing…
Post Comment
Edit your comment

12.2 12.2 Presentation Transcript

  • Gas Laws 12.2
  • 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.)
  • 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
  • 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
  • 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
  • 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.