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Unit 1- Thermodynamics  

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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=mHf

  • equation for Heat of Vaporization- q=mHv

  • equation for specific heat capacity- q=mCAT

    • m= mass

    • H= heat (of fusion or vaporization depending on f and v)

    • 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)

CG

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=mHf

  • equation for Heat of Vaporization- q=mHv

  • equation for specific heat capacity- q=mCAT

    • m= mass

    • H= heat (of fusion or vaporization depending on f and v)

    • 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)

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