Day 3: Phases & Gases Flashcards
Physical Transition
Phase changes
Chemical Transition
Combustion, changes the element
Solid –> liquid
Fusion (endo)
Liquid –> gas
Vaporization (endo)
Solid –> Gas
Sublimation (endo)
Gas –> Liquid
Condensation (exo)
Liquid –> solid
crystalization (exo)
Gas –> Solid
deposition (exo)
Endothermic reactions
Positive entropy
positive enthalpy
Exothermic reactions
Negative entropy
Negative enthalpy
At the b.p. the atm equals the
vapor pressure
Triple point
solid, liquid & gas meet
Critical point
no more phase changes
Ideal gas assumptions
- Gas molecules themselves have no volume (good @ low pressure)
- No inter molecular attractions between molecules (all collisions are ellastic) (Good @ high temperatures)
Kinetic Energy Average is ∝
to Temperature
Not all molecules move at the same speed
STP (standard temperature and pressure)
1 atm
0 dregrees celcius = 273 K
Units for gases
l L = 1 cm^3 = 1 mL
Kelvin for temperature
Pressure: 1 atm = 760 torr = 760 mmHg = 101325 Pa
Energy: 8.314 J/mol * K OR 0.08206 Latm/molK
n = # mols of gas
> Mass per volume
more dense
Ideal gas law
PV=nRT (works best at low P, high T, and for non-polar gases)
Boyle’s Law
P∝ 1/V
Charle’s Law
V ∝ T, density decreases
Avogadro’s Law
V ∝ n, 6.02 * 10^23 avoardo’s number
Dalton’s partial pressure
Ptot = Pa+Pb..
Pa = XaPtot, Xa= mol fraction
Grham’s Law of Effusion
r1/r2 = √M2/M1
Gases escape through narrow holes
Lighter gas fraction moves faster