Unit 1- Thermodynamics
DO NOT CLICK FLASHCARDS FROM HERE (OR STUDY) Click Here.
Click here for elements flashcards
Phases
Solid- Crystalline structure, non-compressible
Liquid- no structure, but touching, non-compressible
Gas- No structure, spread out, compressible.
Physical properties:
→Properties that can be used to identify the substance(element)
Melting point- point when a solid becomes a liquid
Boiling point(vaporization)-point when a liquid becomes a gas (BP)
Freezing point(solidification)-point when a liquid becomes a solid (FP)
Density-how closely packed matter is in a given volume
Atomic Radius(Pg 10+11 on reference table)-refers to the space a specific element occupies.
Energy:
Potential energy- stored energy
Kinetic energy- (temperature? Kind of but not really)- energy of the motion of particles
Temperature Units:
Temp is the average measure of kinetic energy.
Celcius
Kelvin- absolute zero (no zeros)
conversion- K= c + 273
Phase Changes:
Endothermic- Absorb heat
Exothermic- release heat
Calculating the change of heat:
water:
Heat of fusion 334 j/g (solid to liquid and back/ melting point)
Heat of Vaporization 2260 j/g (liquid to gas and back/ boiling point)
Specific Heat capacity 4.18 j/k(g) (Changes temp, but not phase)
All on reference table (Physical constants of water)
equation for Heat of fusion- q=mH
f
equation for Heat of Vaporization- q=mH
v
equation for specific heat capacity- q=mCAT
m= mass
H= heat (of fusion or vaporization depending on
f
andv
)C= specific heat capacity
AT = Delta temp (difference in temp)
Gases:
Particles are traveling in straight-line paths and are randomly distributed
No definite shape or volume
Large distances between particles, low densities
Can be compressed
Can be liquified at low temperatures and high pressures
Standard Pressure Temperature: (STP)
Pressure: 1 atm or 101.3 kPa or 760 torr
Temperature: 0 C or 273 K
Boyle’s Law:
relationship between pressure and volume
says that the volume occupied by a gas is inversely proportional to the pressure exerted on the gas
Charles’s Law:
Describes the relationship between volume and temperature
Says that the volume occupied by a gas is directly proportional to the temperature(in kelvin)
equation- V1/T1 = V2/T2
The combined gas law:
combines boyles and charles law
Formula(On back of reference table) - (P1)(V1)/T1 = (P2)(V2)/T2
Kinetic Molecular Theory: (KMT)
gases move in a random, constant, straight line motion (Ideal gas)
Have negligible volume (Ideals gas)
no attraction between particles (Ideal gas)
If gas molecules do collide no energy is lost or gained (Ideal gas)
(none of this is actually true but we pretend it is to make the math work out, that’s why it says “Ideal Gas”)
Ideal Gas Vs. Real Gas:
Ideal Gas - Follows all rules above for gas.
Real Gas - gas molecules do have a volume and weak attractive forces
Real Gasses act more like Ideal gasses when there is a higher temperature, and lower pressure.
Liquids:
Vapor Pressure:
The pressure that vapor exerts when the temperature of a liquid increases.
Vapor pressure has a greater influence on boiling than temperature.
A liquid will boil when its vapor pressure equals the pressure of the liquid above it
Table for vapor pressure is on reference table.
Calorimetry:
heat stored in chemical bonds(like calories in your food)
Food labels are actually kilocalories
Specific heat-the heat required to increase the temperature of a substance by 1 degree
The Specific heat of water is on the reference table
Other: (Things to remember)
The two elements that are liquid at room temperature are Bromium, and mercury
The two elements that sublime at STP are Iodine, and Carbon Dioxide
Sublimation- Solid to gas.
When the volume increases, the pressure decreases.
Next Unit: Unit 1.5 (Add-on to Unit 1)
Unit 1- Thermodynamics
DO NOT CLICK FLASHCARDS FROM HERE (OR STUDY) Click Here.
Click here for elements flashcards
Phases
Solid- Crystalline structure, non-compressible
Liquid- no structure, but touching, non-compressible
Gas- No structure, spread out, compressible.
Physical properties:
→Properties that can be used to identify the substance(element)
Melting point- point when a solid becomes a liquid
Boiling point(vaporization)-point when a liquid becomes a gas (BP)
Freezing point(solidification)-point when a liquid becomes a solid (FP)
Density-how closely packed matter is in a given volume
Atomic Radius(Pg 10+11 on reference table)-refers to the space a specific element occupies.
Energy:
Potential energy- stored energy
Kinetic energy- (temperature? Kind of but not really)- energy of the motion of particles
Temperature Units:
Temp is the average measure of kinetic energy.
Celcius
Kelvin- absolute zero (no zeros)
conversion- K= c + 273
Phase Changes:
Endothermic- Absorb heat
Exothermic- release heat
Calculating the change of heat:
water:
Heat of fusion 334 j/g (solid to liquid and back/ melting point)
Heat of Vaporization 2260 j/g (liquid to gas and back/ boiling point)
Specific Heat capacity 4.18 j/k(g) (Changes temp, but not phase)
All on reference table (Physical constants of water)
equation for Heat of fusion- q=mH
f
equation for Heat of Vaporization- q=mH
v
equation for specific heat capacity- q=mCAT
m= mass
H= heat (of fusion or vaporization depending on
f
andv
)C= specific heat capacity
AT = Delta temp (difference in temp)
Gases:
Particles are traveling in straight-line paths and are randomly distributed
No definite shape or volume
Large distances between particles, low densities
Can be compressed
Can be liquified at low temperatures and high pressures
Standard Pressure Temperature: (STP)
Pressure: 1 atm or 101.3 kPa or 760 torr
Temperature: 0 C or 273 K
Boyle’s Law:
relationship between pressure and volume
says that the volume occupied by a gas is inversely proportional to the pressure exerted on the gas
Charles’s Law:
Describes the relationship between volume and temperature
Says that the volume occupied by a gas is directly proportional to the temperature(in kelvin)
equation- V1/T1 = V2/T2
The combined gas law:
combines boyles and charles law
Formula(On back of reference table) - (P1)(V1)/T1 = (P2)(V2)/T2
Kinetic Molecular Theory: (KMT)
gases move in a random, constant, straight line motion (Ideal gas)
Have negligible volume (Ideals gas)
no attraction between particles (Ideal gas)
If gas molecules do collide no energy is lost or gained (Ideal gas)
(none of this is actually true but we pretend it is to make the math work out, that’s why it says “Ideal Gas”)
Ideal Gas Vs. Real Gas:
Ideal Gas - Follows all rules above for gas.
Real Gas - gas molecules do have a volume and weak attractive forces
Real Gasses act more like Ideal gasses when there is a higher temperature, and lower pressure.
Liquids:
Vapor Pressure:
The pressure that vapor exerts when the temperature of a liquid increases.
Vapor pressure has a greater influence on boiling than temperature.
A liquid will boil when its vapor pressure equals the pressure of the liquid above it
Table for vapor pressure is on reference table.
Calorimetry:
heat stored in chemical bonds(like calories in your food)
Food labels are actually kilocalories
Specific heat-the heat required to increase the temperature of a substance by 1 degree
The Specific heat of water is on the reference table
Other: (Things to remember)
The two elements that are liquid at room temperature are Bromium, and mercury
The two elements that sublime at STP are Iodine, and Carbon Dioxide
Sublimation- Solid to gas.
When the volume increases, the pressure decreases.