Test 7 Flashcards
(19 cards)
Kinetic Theory of Matter
Kinetic Theory of Matter: explains the existence of states of matter by how far particles are spread from each other and how much they’re moving
Temperature: average kinetic energy of a system
Absolute zero: zero movement
solid
substances whose particles are very closely packed and vibrating gently back and forth
liquid
substances whose particles are further apart and “slipping and sliding” around each other
gas
substances whose particles are very far apart and zipping around quickly
Melting
solid to liquid
Particles gain enough kinetic energy to break away from each other and move more
Melting point: temperature at which this transition occurs
Freezing
liquid to solid
Particles lose enough kinetic energy and form a densely packed formation and move less
Freezing point: temperature at this transition
Vaporization
liquid to gas
Boling: when vapor pressure of the liquid exceeds the atmosphere pressure
Vapor pressure: tendency of liquids to go into the gas phase
Evaporation: only occurs on the surface of a liquid. Particles gain enough kinetic energy to break away
Condensation
gas to liquid
Gas particles lose enough kinetic energy to come together like a liquid
Sublimation
solid to gas
Solid transitions directly into gas phase without passing through liquid phase (ex: dry ice)
Deposition
gas to solid
Ex: dry ice
Molar Heat of Fusion (ΔHfus)
Amount of energy needed to change 1 mole of a solid to a liquid (or vice versa) at its melting/freezing point
Molar Heat of Vaporization(ΔHvap)
Amount of energy needed to change 1 mole of a liquid to a gas ( or vice versa) at its boiling/condensation point
Dalton’s Law of Partial Pressure
Total pressure of a mixture of gases is equal to the sim of partial pressures of each gas
Ptotal = Pa + Pb + Pc … + Pn
Boyle’s Law
At a constant temperature the pressure of a gas is inversely proportional to its volume
PiVi = PfVf
Charles Law
At a constant pressure, the volume of a gas is directly proportional to its temperature
Vi/Ti = Vf/Tf
Gay-Lussac’s Law
At a constant volume, the pressure of a gas is directly proportional to its temperature
Pi/Ti = Pf/Tf
Combined Gas Law
Mathematic relationship between pressure, temperature and volume
PiVi/Ti = PfVf/Tf
Molar Volume
22.4 L/mol
Ideal Gas Law
PV=nRT
