Reading...
Play button
Play button
Use LEFT and RIGHT arrow keys to navigate between flashcards;
Use UP and DOWN arrow keys to flip the card;
H to show hint;
A reads text to speech;
29 Cards in this Set
- Front
- Back
|
Kinetic Energy
|
Energy created by movement
|
|
|
Kinetic Theory
|
All particles are in constant motion
|
|
|
Gas particles
|
small, indefinite volume, particles in random, rapid motion, particles collide with each other
|
|
|
Elastic collision
|
Kinetic energy is completely transferred from one object to another; Total kinetic energy of the system is conserved
|
|
|
Gas pressure
|
a force experienced when gas particles collide with each other
|
|
|
Atmospheric pressure
|
collision of particles in the air with another object
|
|
|
Convert from atm = mmHg = kPa
|
1 atm = 760 mmHg = 101.3 kPa
|
|
|
How are the average kinetic energy and Kelvin temperature related?
|
Directly proportional (if one increases by a factor of 2, the other also increases by a factor of 2, vice versa)
|
|
|
How does the kinetic energy in liquid particles compare to the kinetic energy in gas particles?
|
Kinetic energy in liquid particles is lower due to the intermolecular attraction between liquid particles
|
|
|
Liquid particles
|
takes the shape of the container, volume not affected by pressure, denser than gas particles
|
|
|
Evaporation
|
transition between liquid and gas; when liquid particles meet the minimum required kinetic energy to convert to gas
|
|
|
Vapor pressure
|
force exerted by gas particles on the liquid (area right above liquid)
|
|
|
Dynamic equilibrium
|
rate of evaporation = rate of condensation; no net change of particles in the system
|
|
|
What happens to vapor pressure as temperature increases?
|
Vapor pressure increases as well because the kinetic energy increases as temperature increases so more liquid particles are able to convert to gas particles
|
|
|
STP (Standard Temperature Pressure) Conditions
|
1 mole = 22.4L;
0 degrees Celcius = 273 Kelvin 1 atm = 101.3 kPa = 760 mmHg |
|
|
Boiling point
|
a temperature where ALL of the liquid particles have enough kinetic energy to convert into gas (evaporate)
|
|
|
Normal Boiling Point
|
boiling point of a substance at STP
|
|
|
If you are at an area with elevated atmospheric pressure, will you have a higher or lower boiling point?
|
Higher boiling point because more kinetic energy is required to meet the elevated atmospheric pressure
|
|
|
Solid particles
|
very condensed, not compressible, pressure has no effect on the volume, no/little movement of particles, very low kinetic energy
|
|
|
Melting point
|
temperature where there is enough kinetic energy to break up the solid bonds to they can melt in to liquid particles; same as FREEZING POINT
|
|
|
What factor determines the melting/freezing point of a solid?
|
The type of bonds - the stronger the bonds (ionic bonds), more energy is required to break them --> higher melting /freezing point
|
|
|
Crystals
|
particles that are arranged in an organized, ordered manner
|
|
|
Unit cell
|
the smallest group of a crystal that retains the structure of the crystal
|
|
|
Allotropes
|
different structures, same elements
|
|
|
Amorphous solids
|
solid that lacks order (opposite of a crystal)
|
|
|
Sublimation
|
directly from solid to gas
|
|
|
When does sublimation occur?
|
when the vapor pressure of the solid is greater than atmospheric pressure
|
|
|
Triple Point
|
point where substance exist in solid, liquid, AND gas
|
|
|
What do the solid lines in a phase diagram represent
|
The temperature and pressure at which a substance can shift phases
|
