# Chemistry Chapter 11 Gases

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1. Kinetic Molecular Theory of Gas
• Particles are separated by large distances
• They are in random motion
• They do not form attractive or repulsion forces on one another
• Avg Kinetic Energy α absolute temp
• so T ↑, Ek↑
2. p = force/area
gas particles colliding with walls of the container
3. remember this formula
P1V1/T1 = P2V2/T2

PV = nRT
4. Boyle's Law
relationship b/t P and V

P1V1 = P2V2

@ constant T
5. Charles Law
• Volume and Temperature @ constant pressure
• V1/T1 = V2/T2

As Temp increases, Volume increases (proportional)

*Always use kelvin
6. C to Kelvin
K = C + 273.15
moles (n) and volume relationship

v1/n1 = v2/n2

so P1V1/n1T1 = P2V2/n2T2
8. Ideal Gas Equation Law
PV = nRT

R is gas constant = .08206 L-atm/molar K
9. Standard Temp and Pressure (STP)
1 mol of gas at 0C (273.15K) + 1 atm

PVnRT (solve for V)

V = nRT/P
10. 1 mol gas @ STP
22.414L
11. Dalton's Law of Partial Pressure

Gas Mixtures
• Ptotal = ΣPi
• Ptotal = Pn + Po + Par
12. Mole Fractions (Xi)
Tells the relative amounts of a gas mixture

• Xi = ni/ntotal
• (no units)
13. Consider the following regarding Mole Fractions
• 1. Mole fraction of a component is < 1
• 2. Sum of mole fractions for all components = 1
• 3. Mole fraction is dimensionless

Xi = Pi/Ptotal
 Author: misol ID: 301814 Card Set: Chemistry Chapter 11 Gases Updated: 2015-04-30 04:31:05 Tags: chemistry sacco wake tech Folders: Description: chemistry sacco wake tech Show Answers: