10-3 - Chapters 2 - 6: examined components Chapters 7:...

Info iconThis preview shows pages 1–11. Sign up to view the full content.

View Full Document Right Arrow Icon
Chapters 2 - 6:  examined components Chapters 7:  examine bulk properties Gases 
Background image of page 1

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full DocumentRight Arrow Icon
Gas Laws variable:  amount  (n) unit:  mole (mol) Ideal Gas Law Constant: R R = 0.0821 atm•L K•mol Variables of state and their units: variable:  pressure (P) unit:  atmosphere (atm) variable:  volume (V) unit:  liter (L) conversion factors: variable:  temperature (T) unit:  Kelvin (K) conversion factor: K = o C + 273 1 atm 760 mm Hg 1 atm 760 torr Section 7.1
Background image of page 2
766 mm Hg H = + 18 mm Section 7.1 Trapped gas is greater/less than 766 mm Hg? It’s pushing harder = 784 mm Hg +
Background image of page 3

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full DocumentRight Arrow Icon
766 mm Hg H = 25 mm Section 7.1 Trapped gas is greater/less than 766 mm Hg? It’s not  Pushing as hard = 741 mm Hg -
Background image of page 4
766 mm Hg H = 12 mm What is the pressure of the gas in the bulb? How do I get that pressure from mm Hg to atmospheres? Section 7.1
Background image of page 5

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full DocumentRight Arrow Icon
Ideal Gas Law PV = nRT PV = nRT Keep constant P i V i = P (8 atm) (4 atm)(4 L) = 16 atm•L V (2 L) 16 atm•L Inversely proportional Boyle’s Law Section 7.1 Demo: the belljar balloon And the Cartesian Diver
Background image of page 6
Directly proportional Charles’ Law V i T i 4 L 1 L/K 4 K V f 8 L 1 L/K = 8 K = T f Ideal Gas Law PT PT V = nR P T PV = nRT Keep constant PV = nRT Section 7.1 Demo: balloon and  N 2
Background image of page 7

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full DocumentRight Arrow Icon
Absolute Temperature The temperature at which any number of moles of  gas has a volume of ZERO is O Kelvin (Otherwise known as –273.15 C) Section 7.1
Background image of page 8
Directly proportional V x n x 11.2 L 22.4 L/mol 0.5 mol V z 22.4 L 22.4 L/mol = 1 mol = n z Avagadro’s Law Ideal Gas Law Pn Pn V = RT P n PV = nRT Keep constant PV = nRT Section 7.1 Demo: blowing a  balloon up
Background image of page 9

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full DocumentRight Arrow Icon
Keep constant VT TV P = nR V T Ideal Gas Law PV = nRT Section 7.1 P i T i
Background image of page 10
Image of page 11
This is the end of the preview. Sign up to access the rest of the document.

Page1 / 28

10-3 - Chapters 2 - 6: examined components Chapters 7:...

This preview shows document pages 1 - 11. Sign up to view the full document.

View Full Document Right Arrow Icon
Ask a homework question - tutors are online