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Thermodynamics
honors chem
| Term | Definition |
|---|---|
| thermodynamics | area of physics/chemistry that relates to heat, temperature, and energy. it is used to measure energy absorbed, released, and transferred in a system. |
| kinetic energy | energy related to the MOTION of the atoms. |
| thermal energy | the greater the motion of the particles, the more heat they will produce |
| the average kinetic energy in a system = | temperature |
| potential energy | stored energy |
| chemical energy | the energy stored in bonds caused by attractive forces between electrons (-) and protons (+). the ions attraction have stored energy |
| First Law of Thermodynamics | - energy of a system is constant - energy cannot be created or destroyed, only transferred |
| describe the change in energy when bonds are broken | stable, LOW energy to HIGH energy give energy ex) NaCl --> Na + Cl |
| describe the change in energy when bonds are formed | HIGH energy to LOW energy looses/releases energy big explosion from potential energy ex) Na + Cl --> NaCl + energy |
| Second Law of Thermodynamics | -heat cannot flow from a colder location to a hotter location - energy (heat) flows from hot to cold |
| describe the heat of flow between the air, beaker, and a cup of ice water | From the air, to the beaker, to the ice water |
| Describe the heat flow between your hand, a cup of coffee, and the room | from the cup of coffee, to your hand, to the room |
| Third Law of Thermodynamics | - absolute zero is the point at which all energy = 0 - all motion stops (KE=0, PE=0) |
| have we ever reached absolute zero? | no it is theoretical |
| Celsius is based upon | water |
| Fahrenheit is based upon | not water |
| boiling/freezing point of water in C and F | 100 C & 0 C 212 F &32 F |
| kelvin is an | absolute energy scale |
| enthalpy | heat |
| exothermic | - energy EXITS into the surroundings (we measure in terms of the surroundings). system looses energy - energy is a product - beaker/thermometer gets warm, flame/light/hear produced - potential --> kinetic - ex) hot pack |
| endothermic | - energy ENTERS into the system. surroundings loose energy =cold - energy is a reactant - ex) cold pack - u need heat from a hot plate to start the reaction - the reaction becomes cold as it removes heat from the surroundings - kinetic --> potential |
| is freezing exo or endo? | Exo |
| is boiling/vaporization/evaporation exo or endo? | endo |
| condensation | g --> l |
| is condensation exo or endo? | exo |
| is melting exo or endo? | endo |
| sumblimation | s --> g |
| is sublimation exo or endo? | endo |
| deposition | g --> s |
| is deposition exo or endo? | exo |
| crystalization/freezing/melting | heat of fusion |
| condensation/boiling | heat of vaporization |
| heats of vaporization and fusion are only used when calculating the amount of energy in the | PHASE CHANGE (plateau on the graph) |
| mcat formula is only used when calculating the amount of energy used during a | TEMPERATURE CHANGE (increase/decrease parts on the graph) |
| specific heat capacity | the measure of energy absorbed for every 1g/degree C |
| low specific heat capacity means... | - they conduct heat easily - heat up and cool down FAST - metals |
| high specific heat capacity means ... | - they don't conduct heat easily - heat up and cool down SLOW - ex) water (4.18) |
| things with low specific heats are good... | insulators ex) (non metals) water, glass, fiber glass, air, Styrofoam, wood |
| calorimeter | an insulated container which prevents the flow of heat in or out to the surroundings. |
| you might need to convert kilograms to grams. just remember... | 1000g/1kg |
| conversions c to f/f to c | C= 5/9 (F-32) F= 9/5 C + 32 |
| conversions c to K / K to c | C = K-173 K = C + 173 |
Created by:
deckerc0305